1. The document contains a chemistry practice problems document from Etoos Academy with questions on topics including the mole concept, stoichiometry, gas laws, and periodic properties.
2. It provides 10 questions each on 4 separate daily practice problem sheets related to chemistry, with an answer key provided at the end.
3. The questions are meant to prepare students for the JEE Advanced chemistry exam in 2015 and cover various fundamental concepts tested on this exam.
1. The document provides a chemistry practice problems document (DPP) containing multiple choice questions.
2. The DPP covers topics such as chemical equilibrium, equilibrium constants, reaction stoichiometry, and thermochemistry.
3. The document includes the answer key for the 10 questions in DPP No. 15 and the 10 questions in DPP No. 14, providing the correct option for each multiple choice question.
The document contains daily practice problems for chemistry. It includes two sets of problems (DPP No. 03 and DPP No. 04) targeting the JEE Advanced exam in 2014. Each set contains around 10 single-choice or fill-in-the-blank questions related to stoichiometry, chemical equations, average atomic/molecular mass calculations, and percentage yield. The questions are followed by an answer key providing the correct options.
(i) The document provides 15 solubility product (Ksp) problems involving calculation of solubility, concentration of ions, and value of Ksp for various salts.
(ii) It also provides 12 additional problems involving effect of common ions on solubility, calculation of solubility in presence of other salts, and percentage saturation.
(iii) The problems cover concepts including dissociation of salts into ions, calculation of solubility and concentration using Ksp expression, and effect of common ions in altering solubility.
Some basic concepts of chemistry exercise with solutionssuresh gdvm
This document contains sample questions and answers from Class 11 chemistry Chapter 1 on basic chemistry concepts. The questions calculate molecular masses, empirical and molecular formulas, mass percentages of elements in compounds, moles of reactants and products in chemical reactions, molarity and molality calculations. It also defines terms like significant figures, pressure, mass and prefixes related to the International System of Units.
The document contains 50 multiple choice questions from a 1st year chemistry notes chapter on basic concepts. The questions cover topics like atoms, molecules, ions, isotopes, relative atomic mass, and stoichiometry calculations.
The document also includes the answers to all 50 questions at the end.
The document contains a foundation course on matter in our surroundings from CBSE. It includes 11 multiple choice questions about the properties of solids, liquids, and gases. It then has an objective test section with fill-in-the-blank, true/false, and multiple choice questions related to states of matter, phase changes, density, temperature scales, and other concepts. The questions assess understanding of key ideas like the differences between solids, liquids, and gases, properties like compressibility and thermal conduction, and processes like evaporation, diffusion, and sublimation.
This document contains 50 multiple choice questions from a 1st year chemistry notes chapter on basic concepts. The questions cover topics like atoms, molecules, ions, isotopes, relative atomic mass, stoichiometry, moles, the mole concept, and gas laws. An answer key is provided at the end with the correct response for each question.
This document appears to be an exam for a chemistry course. It contains 27 multiple choice questions testing concepts related to intermolecular forces, phase diagrams, solutions, and chemical kinetics. The key at the bottom provides the correct answer for each question.
1. The document provides a chemistry practice problems document (DPP) containing multiple choice questions.
2. The DPP covers topics such as chemical equilibrium, equilibrium constants, reaction stoichiometry, and thermochemistry.
3. The document includes the answer key for the 10 questions in DPP No. 15 and the 10 questions in DPP No. 14, providing the correct option for each multiple choice question.
The document contains daily practice problems for chemistry. It includes two sets of problems (DPP No. 03 and DPP No. 04) targeting the JEE Advanced exam in 2014. Each set contains around 10 single-choice or fill-in-the-blank questions related to stoichiometry, chemical equations, average atomic/molecular mass calculations, and percentage yield. The questions are followed by an answer key providing the correct options.
(i) The document provides 15 solubility product (Ksp) problems involving calculation of solubility, concentration of ions, and value of Ksp for various salts.
(ii) It also provides 12 additional problems involving effect of common ions on solubility, calculation of solubility in presence of other salts, and percentage saturation.
(iii) The problems cover concepts including dissociation of salts into ions, calculation of solubility and concentration using Ksp expression, and effect of common ions in altering solubility.
Some basic concepts of chemistry exercise with solutionssuresh gdvm
This document contains sample questions and answers from Class 11 chemistry Chapter 1 on basic chemistry concepts. The questions calculate molecular masses, empirical and molecular formulas, mass percentages of elements in compounds, moles of reactants and products in chemical reactions, molarity and molality calculations. It also defines terms like significant figures, pressure, mass and prefixes related to the International System of Units.
The document contains 50 multiple choice questions from a 1st year chemistry notes chapter on basic concepts. The questions cover topics like atoms, molecules, ions, isotopes, relative atomic mass, and stoichiometry calculations.
The document also includes the answers to all 50 questions at the end.
The document contains a foundation course on matter in our surroundings from CBSE. It includes 11 multiple choice questions about the properties of solids, liquids, and gases. It then has an objective test section with fill-in-the-blank, true/false, and multiple choice questions related to states of matter, phase changes, density, temperature scales, and other concepts. The questions assess understanding of key ideas like the differences between solids, liquids, and gases, properties like compressibility and thermal conduction, and processes like evaporation, diffusion, and sublimation.
This document contains 50 multiple choice questions from a 1st year chemistry notes chapter on basic concepts. The questions cover topics like atoms, molecules, ions, isotopes, relative atomic mass, stoichiometry, moles, the mole concept, and gas laws. An answer key is provided at the end with the correct response for each question.
This document appears to be an exam for a chemistry course. It contains 27 multiple choice questions testing concepts related to intermolecular forces, phase diagrams, solutions, and chemical kinetics. The key at the bottom provides the correct answer for each question.
This document contains a practice test for Exam 2 covering Chapters 3, 4, and 7 of a chemistry course. The test has 30 multiple choice questions testing concepts like balancing chemical equations, stoichiometry, gas laws, solution concentrations, acid-base reactions, and periodic trends. The key is provided with the letter answers for each question.
MCAT CHEMISTRY SOLVED PAST PAPERS (2008-2016) - Malik XufyanMalik Xufyan
This document contains 100 multiple choice questions from past MCAT Chemistry papers from 2008-2009. The questions cover various topics in chemistry including bonding, reactions, stoichiometry, states of matter, thermodynamics and organic chemistry. This review material is intended to help students prepare for the MCAT entrance exam by practicing with prior year exam questions.
This document discusses chemical bonding and dipole moments. It contains questions about the units of dipole moment, molecules with zero dipole moment, factors that determine whether a molecule has a dipole moment, and bond properties like bond length, bond energy, and hybridization.
1st year chemistry full book short question ansMalik Xufyan
The document discusses short questions from a first chapter chemistry exam. It includes definitions of terms like ions, gram atoms, and molar volume. It also answers questions about atomic masses of elements, the law of conservation of mass in stoichiometry, limiting reactants in chemical reactions, and how Avogadro's number explains the stoichiometry of reactions involving acids and bases.
1. The document contains a practice test with multiple choice questions about chemical kinetics and equilibrium.
2. Questions cover topics like reaction rates, rate laws, reaction orders, equilibrium constants, Le Chatelier's principle, and the Haber process.
3. There is also a bonus section with chemical nomenclature questions matching names to formulas.
ANURAG TYAGI CLASSES (ATC) is an organisation destined to orient students into correct path to achieve
success in IIT-JEE, AIEEE, PMT, CBSE & ICSE board classes. The organisation is run by a competitive staff comprising of Ex-IITians. Our goal at ATC is to create an environment that inspires students to recognise and explore their own potentials and build up confidence in themselves.ATC was founded by Mr. ANURAG TYAGI on 19 march, 2001.
This document provides information about stoichiometry and fundamental chemistry concepts. It discusses chemical reactions and equations, including types of reactions like combustion, decomposition, and double displacement. Five fundamental chemical laws are explained: conservation of mass, definite proportions, multiple proportions, combining volumes, and Avogadro's hypothesis. Concepts like mole, molecular mass, and formula mass are defined. Worked examples demonstrate how to use these concepts to calculate quantities in chemical reactions from mass and volume relationships.
1st year chemistry 1st chapter short question answers - Malik XufyanMalik Xufyan
This document contains answers to questions about chemistry concepts such as ions, stoichiometry, limiting reactants, atomic mass, and moles. It defines terms like gram atom, gram molecular mass, molar volume, and Avogadro's number. It provides examples to illustrate concepts like how one mole of H2SO4 requires two moles of NaOH for complete neutralization due to each having different numbers of ions. Overall it concisely explains chemistry concepts and uses examples to show how concepts like moles, atoms, and reactions relate based on principles such as the law of conservation of mass.
PPSC CHEMISTRY PAST PAPERS MCQS solved BY Malik XUFYANMalik Xufyan
This document contains a chemistry past paper with multiple choice questions from JIAS Academy. It includes 61 multiple choice questions testing concepts in chemistry such as atomic structure, chemical bonding, redox reactions, acid-base reactions, and organic chemistry. The questions are from a practice test intended to help students prepare for the PPSC chemistry exam.
First Year Chemistry_Full Book Exercise Mcqs SolvedMalik Xufyan
- The document contains sample multiple choice questions from the 1st Year Chemistry textbook covering topics like basic concepts, experimental techniques, gases, liquids and solids, atomic structure, and chemical bonding.
- Questions are provided from chapters 1-6 of the textbook along with four answer options for each question.
- The purpose of the document is to provide a full book of sample exercise MCQs for 1st Year Chemistry exams for all Punjab boards in Pakistan.
iPositive Academy offers the best NEET Coaching. Score 600+ in NEET entrance exam with training from us. We are the best in NEET UG Coaching Coimbatore http://ipositiveacademy.com/
The document provides examples for calculating the Ksp (solubility product constant) of various ionic compounds given their molar solubility in water. It first explains the general process: writing the dissolution reaction, writing the Ksp expression, inserting concentrations based on molar ratios, and calculating the value. Several examples are then worked through step-by-step, calculating Ksp values from molar solubilities for compounds such as silver bromide, calcium fluoride, and mercury(I) bromide. The document also discusses calculating Ksp from solubilities provided in grams per 100mL by first converting to molar solubility. More examples demonstrate this process for nickel sulfide, magnesium fluoride, and manganese(II) i
Definitions and mcqs of ninth class chemistry (chemical combinations)Dr. Sajid Ali Talpur
This document defines key terms related to chemistry including atomic mass, molecular mass, empirical formula mass, molecular formula, empirical formula, mole, molar mass, and Avogadro's number. It then provides 20 multiple choice questions related to these concepts, with an answer key provided at the end. The questions test understanding of concepts like the law of conservation of mass, empirical formulas of compounds, determining moles and mass in chemical equations and reactions.
This document contains questions about thermodynamics and electronic structure. Regarding thermodynamics, questions cover topics like exothermic and endothermic phase changes, standard enthalpies of formation, entropy, Gibbs free energy, and thermochemical equations. Regarding electronic structure, questions cover topics like electron configurations, quantum numbers, diamagnetism, isoelectronic species, and periodic trends.
This document contains 15 multiple choice questions about thermodynamics and 5 multiple choice questions about electronic structure. The thermodynamics questions cover topics like phase changes, entropy, Gibbs free energy, enthalpy of reaction, and thermochemistry calculations. The electronic structure questions cover topics like electron configuration, quantum numbers, and isoelectronic species.
The document contains 25 multiple choice questions related to chemistry concepts like moles, stoichiometry, redox reactions, and titrations. Some key details include:
- Questions cover various mole calculations, redox reaction types, and titration problems involving molarity, normality and volume calculations.
- Redox questions identify the number of electrons transferred in reactions and whether a reaction involves oxidation or reduction.
- Titration calculations determine volumes of acids and bases needed to reach endpoints or find normalities/molarities based on titration data.
- Other questions involve stoichiometry, gas laws, limiting reactants and products of combustion reactions.
This document contains a 27 question practice test on chemistry topics including:
- Balancing chemical equations
- Identifying limiting reactants and calculating theoretical yields
- Solubility rules
- Concentration calculations
- Acid-base reactions
- Nomenclature
The test covers chapters 3 and 4 of a general chemistry textbook, focusing on stoichiometry, types of chemical reactions, aqueous solutions, and acid-base chemistry. It provides multiple choice questions to assess understanding of these core chemistry concepts.
This document contains two practice problem sets (DPP No. 11 and DPP No. 12) for chemistry. DPP No. 11 contains 9 multiple choice questions related to gas laws, kinetic molecular theory, and real gases. DPP No. 12 contains 7 multiple choice questions also related to gas laws and properties of real gases, including questions on Vander Waals constants and critical temperature. The document provides the multiple choice options for each question, as well as the answer key for DPP No. 11 and DPP No. 12. It is a study resource for the JEE Advanced exam focusing on gas laws and properties of real gases.
1. The document contains updates to content in the NCERT Class 11 Biology textbook, including corrections, additions, and replacements of text, diagrams, and figures.
2. Updates include adding more detail about fungal cell walls, correcting terminology related to algae and viruses, and adding sections on prions and anatomical details of plants and animals.
3. Diagrams are also added or updated regarding biological structures and processes such as ribosomes, protein structure, and mitosis.
The document discusses the boron and carbon family (groups 13-14) of the periodic table. It provides information on their electronic configurations, atomic properties, oxidation states, chemical properties including reactivity with air, acids, bases and halogens. It notes the anomalous properties of boron compared to other family members due to the absence of d-orbitals. Examples of compounds in each group are also given such as borax, boric acid, aluminium chloride and oxides.
This document contains a practice test for Exam 2 covering Chapters 3, 4, and 7 of a chemistry course. The test has 30 multiple choice questions testing concepts like balancing chemical equations, stoichiometry, gas laws, solution concentrations, acid-base reactions, and periodic trends. The key is provided with the letter answers for each question.
MCAT CHEMISTRY SOLVED PAST PAPERS (2008-2016) - Malik XufyanMalik Xufyan
This document contains 100 multiple choice questions from past MCAT Chemistry papers from 2008-2009. The questions cover various topics in chemistry including bonding, reactions, stoichiometry, states of matter, thermodynamics and organic chemistry. This review material is intended to help students prepare for the MCAT entrance exam by practicing with prior year exam questions.
This document discusses chemical bonding and dipole moments. It contains questions about the units of dipole moment, molecules with zero dipole moment, factors that determine whether a molecule has a dipole moment, and bond properties like bond length, bond energy, and hybridization.
1st year chemistry full book short question ansMalik Xufyan
The document discusses short questions from a first chapter chemistry exam. It includes definitions of terms like ions, gram atoms, and molar volume. It also answers questions about atomic masses of elements, the law of conservation of mass in stoichiometry, limiting reactants in chemical reactions, and how Avogadro's number explains the stoichiometry of reactions involving acids and bases.
1. The document contains a practice test with multiple choice questions about chemical kinetics and equilibrium.
2. Questions cover topics like reaction rates, rate laws, reaction orders, equilibrium constants, Le Chatelier's principle, and the Haber process.
3. There is also a bonus section with chemical nomenclature questions matching names to formulas.
ANURAG TYAGI CLASSES (ATC) is an organisation destined to orient students into correct path to achieve
success in IIT-JEE, AIEEE, PMT, CBSE & ICSE board classes. The organisation is run by a competitive staff comprising of Ex-IITians. Our goal at ATC is to create an environment that inspires students to recognise and explore their own potentials and build up confidence in themselves.ATC was founded by Mr. ANURAG TYAGI on 19 march, 2001.
This document provides information about stoichiometry and fundamental chemistry concepts. It discusses chemical reactions and equations, including types of reactions like combustion, decomposition, and double displacement. Five fundamental chemical laws are explained: conservation of mass, definite proportions, multiple proportions, combining volumes, and Avogadro's hypothesis. Concepts like mole, molecular mass, and formula mass are defined. Worked examples demonstrate how to use these concepts to calculate quantities in chemical reactions from mass and volume relationships.
1st year chemistry 1st chapter short question answers - Malik XufyanMalik Xufyan
This document contains answers to questions about chemistry concepts such as ions, stoichiometry, limiting reactants, atomic mass, and moles. It defines terms like gram atom, gram molecular mass, molar volume, and Avogadro's number. It provides examples to illustrate concepts like how one mole of H2SO4 requires two moles of NaOH for complete neutralization due to each having different numbers of ions. Overall it concisely explains chemistry concepts and uses examples to show how concepts like moles, atoms, and reactions relate based on principles such as the law of conservation of mass.
PPSC CHEMISTRY PAST PAPERS MCQS solved BY Malik XUFYANMalik Xufyan
This document contains a chemistry past paper with multiple choice questions from JIAS Academy. It includes 61 multiple choice questions testing concepts in chemistry such as atomic structure, chemical bonding, redox reactions, acid-base reactions, and organic chemistry. The questions are from a practice test intended to help students prepare for the PPSC chemistry exam.
First Year Chemistry_Full Book Exercise Mcqs SolvedMalik Xufyan
- The document contains sample multiple choice questions from the 1st Year Chemistry textbook covering topics like basic concepts, experimental techniques, gases, liquids and solids, atomic structure, and chemical bonding.
- Questions are provided from chapters 1-6 of the textbook along with four answer options for each question.
- The purpose of the document is to provide a full book of sample exercise MCQs for 1st Year Chemistry exams for all Punjab boards in Pakistan.
iPositive Academy offers the best NEET Coaching. Score 600+ in NEET entrance exam with training from us. We are the best in NEET UG Coaching Coimbatore http://ipositiveacademy.com/
The document provides examples for calculating the Ksp (solubility product constant) of various ionic compounds given their molar solubility in water. It first explains the general process: writing the dissolution reaction, writing the Ksp expression, inserting concentrations based on molar ratios, and calculating the value. Several examples are then worked through step-by-step, calculating Ksp values from molar solubilities for compounds such as silver bromide, calcium fluoride, and mercury(I) bromide. The document also discusses calculating Ksp from solubilities provided in grams per 100mL by first converting to molar solubility. More examples demonstrate this process for nickel sulfide, magnesium fluoride, and manganese(II) i
Definitions and mcqs of ninth class chemistry (chemical combinations)Dr. Sajid Ali Talpur
This document defines key terms related to chemistry including atomic mass, molecular mass, empirical formula mass, molecular formula, empirical formula, mole, molar mass, and Avogadro's number. It then provides 20 multiple choice questions related to these concepts, with an answer key provided at the end. The questions test understanding of concepts like the law of conservation of mass, empirical formulas of compounds, determining moles and mass in chemical equations and reactions.
This document contains questions about thermodynamics and electronic structure. Regarding thermodynamics, questions cover topics like exothermic and endothermic phase changes, standard enthalpies of formation, entropy, Gibbs free energy, and thermochemical equations. Regarding electronic structure, questions cover topics like electron configurations, quantum numbers, diamagnetism, isoelectronic species, and periodic trends.
This document contains 15 multiple choice questions about thermodynamics and 5 multiple choice questions about electronic structure. The thermodynamics questions cover topics like phase changes, entropy, Gibbs free energy, enthalpy of reaction, and thermochemistry calculations. The electronic structure questions cover topics like electron configuration, quantum numbers, and isoelectronic species.
The document contains 25 multiple choice questions related to chemistry concepts like moles, stoichiometry, redox reactions, and titrations. Some key details include:
- Questions cover various mole calculations, redox reaction types, and titration problems involving molarity, normality and volume calculations.
- Redox questions identify the number of electrons transferred in reactions and whether a reaction involves oxidation or reduction.
- Titration calculations determine volumes of acids and bases needed to reach endpoints or find normalities/molarities based on titration data.
- Other questions involve stoichiometry, gas laws, limiting reactants and products of combustion reactions.
This document contains a 27 question practice test on chemistry topics including:
- Balancing chemical equations
- Identifying limiting reactants and calculating theoretical yields
- Solubility rules
- Concentration calculations
- Acid-base reactions
- Nomenclature
The test covers chapters 3 and 4 of a general chemistry textbook, focusing on stoichiometry, types of chemical reactions, aqueous solutions, and acid-base chemistry. It provides multiple choice questions to assess understanding of these core chemistry concepts.
This document contains two practice problem sets (DPP No. 11 and DPP No. 12) for chemistry. DPP No. 11 contains 9 multiple choice questions related to gas laws, kinetic molecular theory, and real gases. DPP No. 12 contains 7 multiple choice questions also related to gas laws and properties of real gases, including questions on Vander Waals constants and critical temperature. The document provides the multiple choice options for each question, as well as the answer key for DPP No. 11 and DPP No. 12. It is a study resource for the JEE Advanced exam focusing on gas laws and properties of real gases.
1. The document contains updates to content in the NCERT Class 11 Biology textbook, including corrections, additions, and replacements of text, diagrams, and figures.
2. Updates include adding more detail about fungal cell walls, correcting terminology related to algae and viruses, and adding sections on prions and anatomical details of plants and animals.
3. Diagrams are also added or updated regarding biological structures and processes such as ribosomes, protein structure, and mitosis.
The document discusses the boron and carbon family (groups 13-14) of the periodic table. It provides information on their electronic configurations, atomic properties, oxidation states, chemical properties including reactivity with air, acids, bases and halogens. It notes the anomalous properties of boron compared to other family members due to the absence of d-orbitals. Examples of compounds in each group are also given such as borax, boric acid, aluminium chloride and oxides.
This document contains chemistry practice problems and their solutions from Daily Practice Problems (DPP) Nos. 39-42 provided by Etoos Academy.
The first section contains 18 questions testing the ability to calculate oxidation states and draw structures of various compounds. The second section contains similar questions with answers provided.
The third section provides 10 questions on identifying oxidizing and reducing agents, balancing redox reactions, and calculating equivalent weights from experimental data. Sections four and five continue with additional practice problems on balancing redox reactions and calculating equivalent weights.
1. The document contains two practice problem sets (DPP No. 07 and DPP No. 08) from a chemistry course aimed at preparing students for the JEE Advanced exam.
2. Each problem set contains 10 multiple choice or short answer questions covering topics in quantum mechanics, atomic structure, electron configuration and magnetic properties of elements.
3. The document also provides the answer keys for each problem set with the correct responses identified.
The document contains two practice problem sets (DPP No. 15 and 16) for chemistry covering topics related to atomic structure and spectra. DPP No. 15 contains 10 multiple choice questions related to hydrogen and helium spectra, ionization energies, and Bohr orbits. DPP No. 16 contains additional practice problems related to energy levels of helium ions and wavelengths in atomic spectra. The document provides the questions, answers, and context for daily practice problems targeted at the JEE Advanced exam.
(1) The document contains two practice problem sets (DPP No. 39 and 40) for chemistry, containing multiple choice questions testing concepts such as hybridization, molecular structure, and bonding.
(2) DPP No. 39 contains 10 questions on topics like isostructural species, hybridization in molecules, molecular shapes, and ordering properties of ions and molecules.
(3) DPP No. 40 contains 9 additional questions testing concepts like hybridization, molecular structures of SO3 and resonance in nitrate, and the shape and bonding in molecules like B2H6 and AlCl3.
1. The document contains a chemistry practice problem document with multiple choice questions related to topics like graphite and diamond properties, hybridization, VSEPR theory, and structures of compounds.
2. Questions test the understanding of concepts like hybridization states of boron and effects of lone pairs on molecular geometry based on VSEPR theory.
3. The key at the end provides answers to the multiple choice questions along with explanations for ordering properties of compounds.
This document contains chemistry practice problems related to acid-base titration and buffer solutions. It includes 14 problems in DPP 52, 15 problems in DPP 53, and 14 problems in DPP 54, along with the answer keys. The problems cover various concepts such as calculating pH of acid-base solutions, determining amount of salt needed to prepare a buffer of given pH, and finding pH at different stages of acid-base titration. The document is from Etoos Academy and is part of their daily practice problem series targeted towards the JEE Advanced exam.
The document contains two daily practice problem sets (DPP No. 21 & 22) from the Etoos Academy for a chemistry course targeting the JEE Advanced exam in 2015. It includes 10 multiple choice problems in DPP 21 and 10 in DPP 22 related to topics like ionization energies, electron affinities, ionic radii, electronegativity, and periodic trends. The answer key is provided at the end to check the solutions.
1. The document contains two practice problem sets (DPP No. 50 and 51) containing chemistry questions related to acids, bases, pH, and titration curves.
2. It provides the questions, answers, and additional context including dissociation constants, concentrations, volumes, and temperature for interpreting the questions.
3. Key questions from the passages ask about determining pH, concentrations, volumes, and suitable indicators for titration curves based on the provided chemical and physical conditions.
The document contains two daily practice problem sets (DPPs) containing chemistry questions. DPP #35 asks questions about molecular orbital theory, hybridization, and bonding. DPP #36 asks questions about predicting hybridization of molecules based on their Lewis structures. It also contains questions about exceptions to the octet rule and reasons for diamond's hardness. The document provides the answers to all questions posed in the two DPP sets.
This document contains two daily practice problem (DPP) sets from Etoos Academy for chemistry. DPP No. 19 contains 11 multiple choice questions testing concepts related to ionic radii, atomic structure, and ionization energies. DPP No. 20 contains 4 multiple choice questions testing concepts such as ionization energies, periodic trends, and atomic radii measurements. The document provides an answer key for each DPP set.
1. This document contains two practice problem sets (DPP No. 48 and 49) on physical chemistry topics related to acids and bases, including:
2. Calculating pH, concentrations of ions, and degree of dissociation for solutions of weak acids and bases.
3. Questions involve acids like acetic acid, formic acid, hydrofluoric acid and bases like ammonia and calculating equilibrium constants.
4. The answer key provides the solutions to the questions in the two problem sets. Questions involve calculations for various acid/base equilibria, salt hydrolysis, and other equilibrium chemistry concepts.
This document contains two daily practice problem sets for chemistry. It includes 10 multi-part chemistry problems related to gas laws, properties of gases, and gas stoichiometry. The problems cover topics like the relationship between temperature, pressure, volume and amount of gas; gas densities; and calculations involving gas mixtures. An answer key is provided at the end to check work.
This document provides information about mole concept, oxidation-reduction reactions, and titrations. It begins with defining oxidation and reduction processes and listing examples. Rules for determining oxidation numbers and methods for calculating individual oxidation numbers are outlined. The concepts of oxidizing agents, reducing agents, and disproportionation reactions are explained. The document describes how to balance redox reactions using the ion-electron method in both acidic and basic media. Equivalents, normality, and the law of equivalence are defined. Finally, the document discusses types of titrations and provides a table of common redox titrations.
Assignment s block-elements_jh_sir-4173NEETRICKSJEE
The document contains information about s-block elements and their compounds. It begins with an introduction to the topic and syllabus which covers preparation and properties of oxides, peroxides, hydroxides, carbonates, bicarbonates, chlorides and sulphates of sodium, potassium, magnesium and calcium. It then discusses the anomalous properties of lithium and beryllium compared to other elements in their groups. Finally, it provides details on the preparation and properties of specific compounds of alkali metals such as sodium oxide, sodium peroxide, and potassium superoxide.
The document is a study guide for the topic of Periodic Table & Periodicity. It includes sections on theory, exercises and answers. The theory section covers concepts like the modern periodic law, periodic trends in atomic properties, classification of elements into blocks, and periodic properties. It provides detailed explanations of topics like atomic and ionic radii, ionization energy, electron affinity, oxidation states and more. There are multiple exercises provided after the theory section along with an answer key.
This document contains information about mole concept including:
- The table of contents lists topics such as theory, exercises, answer key, and syllabus on mole concept.
- The syllabus section defines mole concept and lists calculations involving chemical reactions.
- Significant figures rules are provided for determining the number of significant figures in measurements.
- Laws of chemical combination such as definite proportions and multiple proportions are explained.
This document does not provide any substantive information as it only contains the word "Topic" with no further context or details. No meaningful summary can be generated from such a short document that lacks essential details about the topic being discussed. More information would be needed to produce an informative summary.
This document contains information about a gaseous state test or assignment, including:
- The table of contents lists 5 exercises and an answer key.
- The document provides definitions and equations for key concepts in the gaseous state including pressure, temperature, the ideal gas law, Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's hypothesis, and the kinetic molecular theory of gases.
- Real gas behavior is discussed along with the van der Waals equation.
ESR spectroscopy in liquid food and beverages.pptxPRIYANKA PATEL
With increasing population, people need to rely on packaged food stuffs. Packaging of food materials requires the preservation of food. There are various methods for the treatment of food to preserve them and irradiation treatment of food is one of them. It is the most common and the most harmless method for the food preservation as it does not alter the necessary micronutrients of food materials. Although irradiated food doesn’t cause any harm to the human health but still the quality assessment of food is required to provide consumers with necessary information about the food. ESR spectroscopy is the most sophisticated way to investigate the quality of the food and the free radicals induced during the processing of the food. ESR spin trapping technique is useful for the detection of highly unstable radicals in the food. The antioxidant capability of liquid food and beverages in mainly performed by spin trapping technique.
The use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptxMAGOTI ERNEST
Although Artemia has been known to man for centuries, its use as a food for the culture of larval organisms apparently began only in the 1930s, when several investigators found that it made an excellent food for newly hatched fish larvae (Litvinenko et al., 2023). As aquaculture developed in the 1960s and ‘70s, the use of Artemia also became more widespread, due both to its convenience and to its nutritional value for larval organisms (Arenas-Pardo et al., 2024). The fact that Artemia dormant cysts can be stored for long periods in cans, and then used as an off-the-shelf food requiring only 24 h of incubation makes them the most convenient, least labor-intensive, live food available for aquaculture (Sorgeloos & Roubach, 2021). The nutritional value of Artemia, especially for marine organisms, is not constant, but varies both geographically and temporally. During the last decade, however, both the causes of Artemia nutritional variability and methods to improve poorquality Artemia have been identified (Loufi et al., 2024).
Brine shrimp (Artemia spp.) are used in marine aquaculture worldwide. Annually, more than 2,000 metric tons of dry cysts are used for cultivation of fish, crustacean, and shellfish larva. Brine shrimp are important to aquaculture because newly hatched brine shrimp nauplii (larvae) provide a food source for many fish fry (Mozanzadeh et al., 2021). Culture and harvesting of brine shrimp eggs represents another aspect of the aquaculture industry. Nauplii and metanauplii of Artemia, commonly known as brine shrimp, play a crucial role in aquaculture due to their nutritional value and suitability as live feed for many aquatic species, particularly in larval stages (Sorgeloos & Roubach, 2021).
hematic appreciation test is a psychological assessment tool used to measure an individual's appreciation and understanding of specific themes or topics. This test helps to evaluate an individual's ability to connect different ideas and concepts within a given theme, as well as their overall comprehension and interpretation skills. The results of the test can provide valuable insights into an individual's cognitive abilities, creativity, and critical thinking skills
The ability to recreate computational results with minimal effort and actionable metrics provides a solid foundation for scientific research and software development. When people can replicate an analysis at the touch of a button using open-source software, open data, and methods to assess and compare proposals, it significantly eases verification of results, engagement with a diverse range of contributors, and progress. However, we have yet to fully achieve this; there are still many sociotechnical frictions.
Inspired by David Donoho's vision, this talk aims to revisit the three crucial pillars of frictionless reproducibility (data sharing, code sharing, and competitive challenges) with the perspective of deep software variability.
Our observation is that multiple layers — hardware, operating systems, third-party libraries, software versions, input data, compile-time options, and parameters — are subject to variability that exacerbates frictions but is also essential for achieving robust, generalizable results and fostering innovation. I will first review the literature, providing evidence of how the complex variability interactions across these layers affect qualitative and quantitative software properties, thereby complicating the reproduction and replication of scientific studies in various fields.
I will then present some software engineering and AI techniques that can support the strategic exploration of variability spaces. These include the use of abstractions and models (e.g., feature models), sampling strategies (e.g., uniform, random), cost-effective measurements (e.g., incremental build of software configurations), and dimensionality reduction methods (e.g., transfer learning, feature selection, software debloating).
I will finally argue that deep variability is both the problem and solution of frictionless reproducibility, calling the software science community to develop new methods and tools to manage variability and foster reproducibility in software systems.
Exposé invité Journées Nationales du GDR GPL 2024
The debris of the ‘last major merger’ is dynamically youngSérgio Sacani
The Milky Way’s (MW) inner stellar halo contains an [Fe/H]-rich component with highly eccentric orbits, often referred to as the
‘last major merger.’ Hypotheses for the origin of this component include Gaia-Sausage/Enceladus (GSE), where the progenitor
collided with the MW proto-disc 8–11 Gyr ago, and the Virgo Radial Merger (VRM), where the progenitor collided with the
MW disc within the last 3 Gyr. These two scenarios make different predictions about observable structure in local phase space,
because the morphology of debris depends on how long it has had to phase mix. The recently identified phase-space folds in Gaia
DR3 have positive caustic velocities, making them fundamentally different than the phase-mixed chevrons found in simulations
at late times. Roughly 20 per cent of the stars in the prograde local stellar halo are associated with the observed caustics. Based
on a simple phase-mixing model, the observed number of caustics are consistent with a merger that occurred 1–2 Gyr ago.
We also compare the observed phase-space distribution to FIRE-2 Latte simulations of GSE-like mergers, using a quantitative
measurement of phase mixing (2D causticality). The observed local phase-space distribution best matches the simulated data
1–2 Gyr after collision, and certainly not later than 3 Gyr. This is further evidence that the progenitor of the ‘last major merger’
did not collide with the MW proto-disc at early times, as is thought for the GSE, but instead collided with the MW disc within
the last few Gyr, consistent with the body of work surrounding the VRM.
Or: Beyond linear.
Abstract: Equivariant neural networks are neural networks that incorporate symmetries. The nonlinear activation functions in these networks result in interesting nonlinear equivariant maps between simple representations, and motivate the key player of this talk: piecewise linear representation theory.
Disclaimer: No one is perfect, so please mind that there might be mistakes and typos.
dtubbenhauer@gmail.com
Corrected slides: dtubbenhauer.com/talks.html
Describing and Interpreting an Immersive Learning Case with the Immersion Cub...Leonel Morgado
Current descriptions of immersive learning cases are often difficult or impossible to compare. This is due to a myriad of different options on what details to include, which aspects are relevant, and on the descriptive approaches employed. Also, these aspects often combine very specific details with more general guidelines or indicate intents and rationales without clarifying their implementation. In this paper we provide a method to describe immersive learning cases that is structured to enable comparisons, yet flexible enough to allow researchers and practitioners to decide which aspects to include. This method leverages a taxonomy that classifies educational aspects at three levels (uses, practices, and strategies) and then utilizes two frameworks, the Immersive Learning Brain and the Immersion Cube, to enable a structured description and interpretation of immersive learning cases. The method is then demonstrated on a published immersive learning case on training for wind turbine maintenance using virtual reality. Applying the method results in a structured artifact, the Immersive Learning Case Sheet, that tags the case with its proximal uses, practices, and strategies, and refines the free text case description to ensure that matching details are included. This contribution is thus a case description method in support of future comparative research of immersive learning cases. We then discuss how the resulting description and interpretation can be leveraged to change immersion learning cases, by enriching them (considering low-effort changes or additions) or innovating (exploring more challenging avenues of transformation). The method holds significant promise to support better-grounded research in immersive learning.
EWOCS-I: The catalog of X-ray sources in Westerlund 1 from the Extended Weste...Sérgio Sacani
Context. With a mass exceeding several 104 M⊙ and a rich and dense population of massive stars, supermassive young star clusters
represent the most massive star-forming environment that is dominated by the feedback from massive stars and gravitational interactions
among stars.
Aims. In this paper we present the Extended Westerlund 1 and 2 Open Clusters Survey (EWOCS) project, which aims to investigate
the influence of the starburst environment on the formation of stars and planets, and on the evolution of both low and high mass stars.
The primary targets of this project are Westerlund 1 and 2, the closest supermassive star clusters to the Sun.
Methods. The project is based primarily on recent observations conducted with the Chandra and JWST observatories. Specifically,
the Chandra survey of Westerlund 1 consists of 36 new ACIS-I observations, nearly co-pointed, for a total exposure time of 1 Msec.
Additionally, we included 8 archival Chandra/ACIS-S observations. This paper presents the resulting catalog of X-ray sources within
and around Westerlund 1. Sources were detected by combining various existing methods, and photon extraction and source validation
were carried out using the ACIS-Extract software.
Results. The EWOCS X-ray catalog comprises 5963 validated sources out of the 9420 initially provided to ACIS-Extract, reaching a
photon flux threshold of approximately 2 × 10−8 photons cm−2
s
−1
. The X-ray sources exhibit a highly concentrated spatial distribution,
with 1075 sources located within the central 1 arcmin. We have successfully detected X-ray emissions from 126 out of the 166 known
massive stars of the cluster, and we have collected over 71 000 photons from the magnetar CXO J164710.20-455217.
Basics of crystallography, crystal systems, classes and different forms
Dpp 02 mole_concept_jh_sir-3572
1. PAGE NO. # 1
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
CHEMISTRY
DAILY PRACTICE PROBLEMS
D P P
COURSE NAME : UDAY (UB) DATE : 10.06.2013 to 15.06.2013 DPP NO. 01 TO 4
TARGET
JEE (ADVANCED) : 2015
* Marked Questions are having more than one correct option.
DPP No. # 1
1. A quantity of aluminium has a mass of 54.0 g. What is the mass of the same number of magnesium
atoms?
(A) 12.1 g (B) 24.3 g (C) 48 g (D) 97.2 g
2. The charge on 1 gram ions of Al3+
is :
(A)
27
1
NA
e coulomb (B)
3
1
× NA
ecoulomb (C)
9
1
× NA
ecoulomb (D) 3 × NA
ecoulomb
3. The density of water at 4°C is 1.0 × 103
kg m–3
. The volume occupied by one molecule of water is
approximately :
(A) 3.0 × 10–23
mL (B) 6.0 × 10–22
mL (C) 3.0 × 10–21
mL (D) 9.0 × 10–23
mL
4. The number of molecules of water in 333 g of Al2
(SO4
)3
. 18H2
O is :
(A) 18.0 × 6.02 × 1023
(B) 9.0 × 6.02 × 1023
(C) 18.0 (D) 36.0
5. From 392 mg of H2
SO4
, 1.204 × 1021
molecules are removed. How many moles of H2
SO4
are left ?
(A) 2.0 × 10–3
(B) 1.2 × 10–3
(C) 4.0 × 10–3
(D) 1.5 × 10–3
6. In which of the following pairs do 1 gm of each have an equal number of molecules ?
(A) N2
O and CO (B) N2
and C3
O2
(C) N2
and CO (D) N2
O and CO2
Comprehension (Q. No. 7 to 9)
Equal number of atoms are contained in one gram atomic weight of each element, and that the same
number of molecules is found in one gram molecular weight of any compound. The terms gram atomic
weight and gram molecular weight are used to refer to a fixed number (Avogadro's number 6.023 x 1023
) of
particle. The term mole stands for the amount of material which contains these number of particles.
7. If 12 g of C12
has equal number of atoms as Avogadro's number what mass of 2
He4
will contain same
number of atoms ?
(A) 2 g (B) 4 g (C) 6 g (D) 3 g
8. What will be the gram atomic weight of Mg, if 24 g of 12
Mg24
contains 6.023 × 1023
atoms ?
(A) 12 g (B) 36 g (C) 24 g (D) 48 g
9. Compute gram molecular weight of H2
gas if 4 g of H2
gas contains 24.09 × 1023
atoms :
(A) 4 g (B) 3 g (C) 2 g (D) 1 g
2. PAGE NO. # 2
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
10. Fill the blanks in the table. Where NA
is Avogadro number.
Sample
Relative atomic
Mass for the
element
Gram
Atomic
mass of
sample
Moles of
sample
No. of atoms
of sample
Mass removed
from the sample
Mole
removed
atoms
removed
Mass of same no.
of C atom as No. of
atoms present in
the original sample
8 gm O atom 16 _ _ _ _ _ _ _ _ _ 2 gm _ _ _ _ _ _ _ _ _
For Example 16 16 gm ½ mole 2 gm mole 6 gm
230 gm Na 23 46 gm
60 gm Ca 40 1 mole
20 gm He 4 3 mole
56 gm N 14 ½ mole
12 gm Mg 24
128 gm S 32 NA
93 gm P 31
4
NA
2
N3 A
2
NA
8
NA
8
1
DPP No. # 2
1. According to common practice, if you have Avogadro number of Hydrogen then its mass is equal to :
(A) 1 g (B) 2 g (C) 4 g (D) depends on temperature
2. From 64 g oxygen, 11.2 lit. Oxygen gas at S.T.P and 6.02 × 1023
oxygen atoms are removed from the
oxygen container. Find the mass of the oxygen gas left.
(A) zero (B) 32 g (C) 16 g (D) none
3. From the mixture of 4 moles Ca3
(PO4
)2
and 5 moles of P4
O10
and 6 moles of H3
PO3
all the phosphorus
atoms are removed then moles of P4
molecule formed from all these atoms is :
(A) 8.5 (B) 17 (C) 34 (D) 10
4. If a sample of CuSO4
.5H2
O contains 3 moles of oxygen molecule the mole of H-atoms present in the sample is:
(A) 5 (B) 9 (C) 10/3 (D) 20/3
5. Sulphur exist in different allotropic forms like S2
, S6
and S8
etc. If equal weight of three are taken in
separate container then the ratio of number of atoms is :
(A) 1 : 3 : 4 (B) 1 : 1 : 1 (C) 2 : 4 : 3 (D) 1 : 1 : 4
6. Which of the following contains the greatest number of atoms ?
(A) 1.0 g of butane (C4
H10
) (B) 1.0 g of nitrogen (N2
)
(C) 1.0 g of silver (Ag) (D) 1.0 g of water (H2
O)
7. Under the same conditions, two gases have the same number of molecules. They must :
(A) be noble gases. (B) have equal volumes.
(C) have a volume of 22.4 dm3
each. (D) have an equal number of atoms.
8. Agaseous mixture contains CO2
(g) and N2
O(g) in a 2 : 5 ratio by mass. The ratio of the number of molecules
of CO2
(g) and N2
O(g) is :
(A) 5 :2 (B) 2 : 5 (C) 1 : 2 (D) 5 : 4
9. In which of the following pairs do 1 g of each have an equal number of molecules?
(A) N2
O and CO (B) N2
and C3
O2
(C) N2
and CO (D) N2
O and CO2
10. 11.2 L of a gas at STP weights 14.0 g. The gas could be :
(A) N2
O (B) NO2
(C) N2
(D) CO
3. PAGE NO. # 3
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
DPP No. # 3
1. The atomic weight for a triatomic gas is a. The correct formula for the number of moles of gas in its w g is:
(A)
a
w3
(B)
a3
w
(C) 3wa (D)
w3
a
2. 16 g of SOx
occupies 5.6 litre at S.T.P. Assuming ideal gas nature, the value of x is :
(A) 1 (B) 2 (C) 3 (D) none of these
3. Find the relative density of SO3
gas with respect to methane.
4. Vapour density of a gas is 17 then find the weight of 11.2 L. of gas at STP.
5. Compounds of boron with hydrogen are called boranes. One of these boranes has the empirical formula
BH3
and a molecular weight of 28 amu. What is its molecular formula ?
6. Calculate vapour density of a sample containing 10 moles of CO2, 5 moles of SO2 & 400 g of SO3 with
respect to CH4 gas.
7. Calculate total number of carbon atoms in a sample containing 160 g of CH4, 600 g of acetic acid, 340 g of
C3O2 & 360 g of pentane.
8. Match the following :
Column - I Column - II
(A) 49 g H2
SO4
(p) 0.5 mole
(B) 20 g NaOH (q) 1.5 NA
atoms
(C) 11.2 L of CO2
at STP (r) 0.5 NA
molecules
(D) 6.023 × 1023
atoms of Oxygen (s) 2 mole of ‘O’ atom
9. Column - I Column - II
(A) 32 gm each of O2 and S (p) 2 moles of Fe
(B) 2 gram molecule of K3[Fe(CN)6] (q) 3 moles of ozone molecule
(C) 144 gm of oxygen atom (r) one mole
(D) From 168 g of iron 6.023 × 1023 atoms (s) 12 moles of carbon atoms
of iron are removed the iron left
DPP No. # 4
1. An element (A) (at wt = 75) and another element (B) (at. wt. = 25) combine to form a compound. The
compound contains 75% (A) by weight. The formula of the compound will be -
(A) A2B (B) A3B (C) AB3 (D) AB
2. The empirical formula of a compound is CH. Its molecular weight is 78. The molecular formula of the
compound will be -
(A) C2H2 (B) C3H3 (C) C4H4 (D) C6H6
3. Hydrogen and oxygen combine to form H2O2 and H2O containing 5.93% and 11.2% Hydrogen
respectively. The data illustrates-
(A) Law of conservation of mass (B) Law of constant proportions
(C) Law of reciprocal proportions (D) Law of multiple proportions
4. PAGE NO. # 4
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
4. If water samples are taken from sea, rivers, clouds, lake or snow, they will be found to contain H2
and O2 in the fixed ratio of 1 : 8. This indicates the law of -
(A) Multiple proportion (B) Definite proportion
(C) Reciprocal proportion (D) None of these.
5. 1.2 gm of Mg (At. mass 24) will produce MgO equal to -
(A) 0.05 mol (B) 40 gm (C) 40 mg (D) 4 gm
6. One of the following combinations illustrate law of reciprocal proportions-
(A) N2O3, N2O4, N2O5 (B) NaCl, NaBr, NaI (C) CS2, CO2, SO2 (D) PH3, P2O3, P2O5
7. The law of multiple proportions is illustrated by -
(A) Carbon monoxide and carbon dioxide (B) Potassium bromide and potassium chloride
(C) Water and heavy water (D) Calcium hydroxide and barium hydroxide.
8. Column matching :
Column I Column II
(A) CaC2 (p) 106 gm
(B) 2 g-equivalent of Na2CO3 (q) 22.4 L at S.T.P.
(C) 6.02 × 1023
Ne atoms (r) N0 formula units
(D) Mohr’s salt (s) Calcium carbide
(E) Contain 18 gm-atom of N (t) (NH4)2SO4.Fe(SO4).6H2O
ANSWER KEY
DPP No. # 1
1. (C) 2. (D) 3. (C) 4. (B) 5. (A) 6. (D) 7. (B)
8. (C) 9. (C)
DPP No. # 2
1. (A) 2. (B) 3. (A) 4. (D) 5. (A) 6. (A) 7. (B)
8. (B) 9. (D) 10. (C)
DPP No. # 3
1. (B) 2. (B) 3. 5 4. 17 5. B2
H6
6.
58
16
7. 70NA
8. (A) p,r,s (B) p,r (C) p, q, r (D) r 9. (A) p,r (B) p,s (C) q (D) p
DPP No. # 4
1. (D) 2. (D) 3. (D) 4. (B) 5. (A) 6. (C) 7. (A)
8. (A) s (B) p (C) q; (D) (t) (E) t
5. PAGE NO. # 1
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
CHEMISTRY
DAILY PRACTICE PROBLEMS
D P P
COURSE NAME : UDAY (UB) DATE : 24.06.2013 to 29.06.2013 DPP NO. 05 TO 08
TARGET
JEE (ADVANCED) : 2015
* Marked Questions are having more than one correct option.
DPP No. # 05
1. The chloride of a metal contains 71% chlorine by weight and the vapour density of it is 50. The atomic
weight of the metal will be -
(A) 29 (B) 58 (C) 35.5 (D) 71
2. The haemoglobin of most mammals contains approximately 0.33% of iron by mass. The molecular
mass of haemoglobin is 67200. The number of iron atoms in each molecule of haemoglobin is-
(A) 3 (B) 4 (C) 2 (D) 6
3. The formula which represents the simple ratio of atoms in a compound is called -
(A) molecular formula (B) structural formula (C) empirical formula (D) rational formula
4. On analysis, a certain compound was found to contain 254 gm of iodine (at. mass 127) and 80 gm
oxygen (at. mass 16). What is the formula of the compound -
(A) IO (B) I2O (C) I5O3 (D) I2O5
5. 14g of element X combine with 16g of oxygen. On the basis of this information, which of the following
is a correct statement :
(A) The element X could have an atomic weight of 7 and its oxide formula XO
(B) The element X could have an atomic weight of 14 and its oxide the formula X2O
(C) The element X could have an atomic weight of 7 and its oxide is X2O
(D) The element X could have an atomic weight of 14 and its oxide is XO2
6. The law of conservation of mass holds good for all of the following except -
(A) All chemical reactions (B) Nuclear reactions
(C) Endothermic reactions. (D) Exothermic reactions.
Passage (Q. No. 7 to 9)
10 moles of SO2 and 4 moles of O2 are mixed in a closed vessel of volume 2 litres. The mixture
is heated in presence of Pt catalyst. Following reaction takes place :
2SO2(g) + O2(g) 2SO3(g)
Assuming the reaction proceeds to completion.
7. Select the correct statement -
(A) SO2 is the limiting reagent (B) O2 is the limiting reagent
(C) both SO2 and O2 are limiting reagent (D) cannot be predicted
8. Number of moles of SO3 formed in the reaction will be -
(A) 10 (B) 4 (C) 8 (D) 14
9. Number of moles of excess reactant remaining -
(A) 4 (B) 2 (C) 6 (D) 8
6. PAGE NO. # 2
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
DPP No. # 06
Fill in the blank :
1. For the reaction,
2x + 3y + 4z 5w
Initially if 1 mole of x, 3 mole of y and 4 mole of z is taken. If 1.25 mole of w is obtained then % yield of this
reaction is _______.
2. The vapour density of a mixture of gas A (Molecular mass = 40) and gas B (Molecular mass = 80) is 25.
Then mole % of gas B in the mixture would be ________.
3. For the reaction
2A + 3B + 5C 3D
Initially if 2 mole of A, 4 mole of B and 6 mole of C is taken. With 25% yield, moles of D which can be
produced are _________.
Single Correct:
4. Mass of sucrose C12H22O11 produced by mixing 84 gm of carbon, 12 gm of hydrogen and
56 lit. O2 at 1 atm & 273 K according to given reaction, is
C(s) + H2(g) + O2 (g) C12H22O11(s)
(A) 138.5 (B) 155.5 (C) 172.5 (D) 199.5
5. The percentage by mole of NO2 in a mixture of NO2(g) and NO(g) having average molecular mass 34 is :
(A) 25% (B) 20% (C) 40% (D) 75%
6. The minimum mass of mixture of A2 and B4 required to produce at least 1 kg of each product is :
(Given At. mass of 'A' = 10 ; At. mass of 'B' = 120)
5A2 + 2B4 2AB2 + 4A2B
(A) 2120 gm (B) 1060 gm (C) 560 gm (D) 1660 gm
7. 74 gm of a sample on complete combustion gives 132 gm CO2 and 54 gm of H2O. The molecular formula
of the compound may be :
(A) C5H12 (B) C4H10O (C) C3H6O2 (D) C3H7O2
8. An iodized salt contains 0.5 % of NaI. Aperson consumes 3 gm of salt everyday. The number of iodide ions
going into his body everyday is :
(A) 10–4 (B) 6.02 ×10–4 (C) 6.02 × 1019 (D) 6.02 × 1023
9. The mass of Mg3N2 produced if 48 gm of Mg metal is reacted with 34 gm NH3 gas is :
Mg + NH3 Mg3N2 + H2
(A)
3
200
(B)
3
100
(C)
3
400
(D)
3
150
7. PAGE NO. # 3
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
DPP No. # 07
1. The mass of P4O10 produced if 440 gm of P4S3 is mixed with 384 gm of O2 is :
P4S3 + O2 P4O10 + SO2
(A) 568 gm (B) 426 gm (C) 284 gm (D) 396 gm
2. Calculate percentage change in Mavg of the mixture, if PCl5 undergo 50% decomposition.
PCl5 PCl3 + Cl2
(A) 50% (B) 66.66 % (C) 33.33 % (D)Zero'kwU;
3. Statement -1 : 2A + 3B C
4/3 moles of 'C' are always produced when 3 moles of 'A' & 4 moles of 'B' are added.
Statement -2 : 'B' is the liming reactant for the given data.
(A) Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1.
(B) Statement-1 is true, statement-2 is true and statement-2 is NOT the correct explanation for statement-1.
(C) Statement-1 is false, statement-2 is true.
(D) Statement-1 is true, statement-2 is false.
4. The recommended daily dose is 17.6 milligrams of vitamin C (ascorbic acid) having formula C6H8O6.
Match the following. Given : NA = 6 × 1023
Column I Column II
(A) O-atoms present (p) 10–4 mole
(B) Moles of vitamin C in 1 gm of vitamin C (q) 5.68 × 10–3
(C) Moles of vitamin C in 1 gm should be consumed daily (r) 3.6 × 1020
5. The number of carbon atoms present in a signature, if a signature written by carbon pencil weights
1.2 × 10–3 g is :
(A) 12.04 × 1020 (B) 6.02 × 1019 (C) 3.01 × 1019 (D) 6.02 × 1020
6. The average atomic mass of a mixture containing 79 mole % of 24Mg and remaining 21 mole % of 25Mg
and 26Mg , is 24.31. % mole of 26Mg is :
(A) 5 (B) 20 (C) 10 (D) 15
7. The density of a liquid is 1.2 g/mL. There are 35 drops in 2 mL. The number of molecules in one drop
(molar mass of liquid = 70 g/mol) is :
(A) A
1.2
N
35
(B)
2
A
1.2 1
N
35 35
(C) A3
1.2
N
(35) (D) 1.2 NA
8. Sulphur trixoide is prepared by the following two reactions
S8(s) + 8 O2(g) 8 SO2(g) ; 2SO2(g) + O2(g) 2SO3(g)
How many grams of SO3 are produced from 1 mol of S8?
(A) 1280.0 (B) 640.0 (C) 960.0 (D) 320.0
9. A compound of Mg contains 6% of Mg then find the minimum molar mass of compound.
8. PAGE NO. # 4
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
DPP No. # 08
1. Vapour density of equimolar mixture of CH4, O2 and SO2 is :
(A) 18.67 (B) 16 (C) 36 (D) 37.3
2. If law of conservation of mass was to hold true, then 20.8 gm of BaCl2 on reaction with 9.8 gm of
H2SO4 will produce 7.3 gm of HCl and BaSO4 equal to -
(A) 11.65 gm (B) 23.3 gm (C) 25.5 gm (D) 30.6 gm
3. A sample contains 9.81 g Zn, 1.8 × 1023 atoms of Cr and 0.6 g-atoms of O. What is empirical formula of
compound ? (Zn = 65 g/mol)
4. If 240 g of carbon is taken in a container to convet it completely to CO2 but in industry it has been found that
280 g of CO was also formed along with CO2. Find the percentage yield of CO2. The reaction occurring are
C + O2 CO2 ; C +
1
2
O2 CO
(A) 25% (B) 50% (C) 75% (D) 100%
5. 100 g impure CaCO3 on heating gives 5.6 lit. CO2 gas at STP. Find the percentage of calcium in the lime
stone sample. [At wt. : Ca = 40 ; C = 12 ; O = 16]
(A) 10 (B) 20 (C) 1 (D) 30
Match the column
6. One type of artifical diamond (commonly called YAG for yttrium aluminium garnet) can be represented by
the formula Y3Al5O12.[Y = 89, Al =27]
Column I Column II
Element Weight percentage
(A) Y (p) 22.73%
(B) Al (q) 32.32%
(C) O (r) 44.95%
7. Butane, C4H10, burns with the oxygen in air to give carbon dioxide and water.
What is the amount (in moles) of carbon dioxide produced from 0.15 mole C4H10?
C4H10(g) + O2(g) CO2(g) + H2O(g) (not balanced)
Answer Key
DPP No. # 5
1. (A) 2. (B) 3. (C) 4. (D) 5. (C) 6. (B) 7. (B)
8. (C) 9. (B)
DPP No. # 06
1. 50% 2. 25% 3. 0.75 4. (B) 5. (A) 6. (A) 7. (C)
8. (C) 9. (A)
DPP No. # 07
1. (B) 2. (C) 3. (C) 4. (A) r, (B) q, (C) p 5. (B) 6. (C)
7. (C) 8. (B) 9. 400 g/mole
DPP No. # 08
1. (A) 2. (B) 3. ZnCr2O4 4. (B) 5. (A)
6. (A) r, (B) p, (C) q
7. 0.6
9. PAGE NO. # 1
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
CHEMISTRY
DAILY PRACTICE PROBLEMS
D P P
COURSE NAME : UDAY (UB) DATE : 01.07.2013 to 06.07.2013 DPP NO. 09 TO 10
TARGET
JEE (ADVANCED) : 2014
* Marked Questions are having more than one correct option.
DPP No. # 09
1. 84 g of iron (Fe) is reacted with sufficient amount of steam to produced 44.8 lit., H2 gas at S.T.P.
according the following reaction, a Fe + b H2O c Fe3O4 + d H2. The stoichiometric coefficients
of the reaction is (Atomic wt. : Fe = 56, O = 16, H = 1)
(A) 4, 3, 1, 4 (B) 3, 4, 1, 4 (C) 1, 4, 2, 3 (D) None of these
2. If 240 g of carbon is taken in a container to convert it completely to CO2 but in industry it has been
found that 280 g of CO was also formed along with CO2. Find the percentage yield of CO2. The
reactions occuring are :
C + O2 CO2 ; C +
1
2
O2 CO
(A) 25% (B) 50% (C) 75% (D) 100%
3. 120 g Mg was burnt in air to give a mixture of MgO and Mg3N2. The mixture is now dissolved in HCl
to form MgCl2 and NH4Cl, if 107 grams NH4Cl is produced. Then the moles of MgCl2 formed is:
(Atomic wt. : Mg = 24, N = 14, Cl = 35.5)]
(A) 3 moles (B) 6 moles (C) 5 moles (D) 10 moles
4. 100 g impure CaCO3 on heating gives 5.6 litre CO2 gas at STP. Find the percentage of calcium in
the lime stone sample. [Atomic weight : Ca = 40; C = 12 : O = 16]
(A) 10 (B) 20 (C) 1 (D) 30
5. 75 mL of H2SO4 (specific gravity = 1.18) containing 49% H2SO4 by mass is diluted to 590 mL.
Calculate molarity of the diluted solution. [S = 32]
(A) 0.7 M (B) 7.5 M (C) 0.75 M (D) 0.25 M
6. Calculte the molarity when :
(a) 4.9 g H2SO4 acid dissolved in water to result 500 mL solution
(b) 2 gram molecule of KOH dissolved in water to result 500 mL solution
7. How would you prepare exactly 3 litre of 1.0 M NaOH by mixing proportions of stock solution of
2.5 M NaOH and 0.4 M NaOH if no water is to be used. Find the ratio of the volume (v1/v2).
8. What volume of 0.25 M HNO3 (nitric acid) reacts with 50 mL of 0.15 M Na2CO3 (sodium carbonate)
in the following reaction?
2HNO3 (aq) + Na2CO3(aq) 2NaNO3 (aq) + H2O() + CO2(g)
10. PAGE NO. # 2
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
9. Zinc and hydrochloric acid react according to the reaction :
Zn(s) + 2HCl (aq) ZnCl2(aq) + H2(g)
If 0.30 mole of Zn are added to hydrochloric acid containing 0.52 mole HCl, how many moles of H2
are produced :
10. Match the following :
Column-I Column-II
For 1 mole of reactant placed in Product
open container in each reaction
(A) PCl5 (g)
PCl3 (g) + Cl2(g) (p) 2NA molecules
(B) CaCO3(s)
CaO(s) + CO2(g) (q) 67.2 litre gaseous product at STP
(C) 2HCl (g)
H2(g) + Cl2(g) (q) 22.4 litre gaseous product at STP
(D) NH4COONH2(s)
2NH3(g) + CO2(g) (s) 44.8 litre gaseous product at STP
DPP No. # 10
1. What volume of a 0.8 M solution contains 100 millimoles of the solute?
(A) 100 mL (B) 125 mL (C) 500 mL (D) 62.5 mL
2. Calculate the volume in litre of 1 M solution of HCl which contain 36.5 g HCl?
3. The molarity of the KOH solution which is containing 2.8% mass-volume solution of KOH is :
(A) M/10 (B) M/2 (C) M/5 (D) 1 M
4. 75 mL of H2SO4 (specific gravity = 1.18) containing 49% H2SO4 by mass is diluted to 590 mL.
Calculate molarity of the diluted solution. [S = 32]
(A) 0.7 M (B) 7.5 M (C) 0.75 M (D) 0.25 M
5*. If 100 mL of 1 M H2SO4 solution is mixed with 100 mL of 9.8% (w/w/) H2SO4 solution (d = 1 gm/
mL) then :
(A) concentration of solution remains same (B) volume of solution become 200 mL
(C) mass of H2SO4 in the solution is 98 gm (D) mass of H2SO4 in the solution is 19.6 gm
6*. For 100 mL of 0.2 M AlCl3 solution + 400 mL of 0.1 M HCl solution correct datas are :
(A) Total concentration of cation (s) = 0.12 M
(B) Total concentration of cation(s) = 0.06 M
(C) [Cl–] = 0.1 M
(D) [Cl–] = 0.2 M
11. PAGE NO. # 3
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,
BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
Comprehension :
Read the following comprehension carefully and answer the questions (Q. 7 to Q. 10)
The concentrations of solutions can be expressed in number of ways ; viz : mass fraction of solute
(or mass percent), Molar concentration (Molarity) and Molal concentration (molality). These terms are
known as concentration terms and also they are related with each other i.e. knowing one concentration
term for the solution, we can find other concentration terms also. The definition of different concentration
terms are given below :
Molarity : It is number of moles of solute present in one litre of the solution.
Molality : It is the number of moles of solute present in one kg of the solvent
Mole fraction =
moles of solute
moles of solute + moles of solvent
If molality of the solution is given as 'a' then mole fraction of the solute can be calculated by
Mole fraction =
solvent
solvent
solvent
a Ma
1000 (a M 1000)
a+
M
where a = molality and Msolvent = Molar mass of
solvent
We can change : Mole fraction Molality Molarity.
7. 120 g of solution containing 40% by mass of NaCl are mixed with 200 g of a solution containing 15%
by mass NaCl. Determine the mass percent of sodium chloride in the final solution :
(A) 24.4% (B) 78% (C) 48.8% (D) 19.68%
8. What is the molality of the above solution ?
(A) 4.4 m (B) 5.5 m (C) 24.4 m (D) None
9. What is the mole fraction of the solute :
(A) 0.18 (B) 0.75 (C) 0.09 (D) 0.25
10. What is the molarity of solution if density of solution in 1.6 g/mL ?
(A) 5.5 M (B) 6.6 M (C) 2.59 M (D) None
ANSWER KEY
DPP No. # 09
1. (B) 2. (B) 3. (C) 4. (A) 5. (C)
6. (a) 0.1 M (b) 4 M 7. 2 : 5 8. 60 mL 9. 0.26
10. (A) p,s (B) p, r (C) r (D) q
DPP No. # 10
1. (B) 2. 1 3. (B) 4. (C) 5*. (ABD)
6*. (AD) 7. (A) 8. (B) 9. (C) 10. (B)