This document contains 49 multiple choice questions covering various chemistry concepts. The questions are formatted as numbered items and include topics such as: electron configurations, lattice energies, gas laws, enthalpy of formation, pH calculations, solubility product constants, and organic reaction mechanisms. For each question, there are typically 4 possible answer choices provided.
IB Chemistry on Born Haber Cycle and Lattice EnthalpyLawrence kok
The document provides information on the Born-Haber cycle and how it can be used to calculate lattice enthalpy for various ionic compounds. It gives step-by-step explanations of standard enthalpy changes used in the Born-Haber cycle calculations for ionic compounds such as LiCl, NaCl, KCl, NaBr, NaF and NaH. Diagrams illustrate the multi-stage process of determining lattice enthalpy values that cannot be measured directly through experimentation.
IB Chemistry on Born Haber Cycle and Lattice EnthalpyLawrence kok
The document describes the Born-Haber cycle process for determining the lattice enthalpy of various ionic compounds such as LiCl, NaCl, KCl, NaBr, NaF, and NaH. The Born-Haber cycle involves breaking down the ionic compound into gaseous ions and then measuring the standard enthalpy changes associated with steps such as atomization, ionization, and electron affinity which are used to calculate the unknown lattice enthalpy value. Diagrams of the Born-Haber cycle are provided for each example compound.
Periodic Table of Elements (Update) by Malik XufyanMalik Xufyan
The document provides a periodic table of the elements with the following information for each element:
1) Atomic number and common ions formed
2) Atomic symbol
3) English element name
4) Atomic mass (rounded)
The periodic table is organized into blocks by orbital type and periods by proton number. Common polyatomic ions are also listed at the bottom with their charge.
Stoichiometry is the quantitative relationship between reactants and products in chemical reactions. Hess's law states that the enthalpy change of a reaction is independent of the pathway and depends only on the initial and final states. Using Hess's law, one can determine the enthalpy change of a reaction by adding the enthalpy changes of multiple steps that combine to give the overall reaction. The standard enthalpy of formation of a compound is the enthalpy change when one mole of the substance is formed from its elements in their standard states.
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.
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The document contains 10 chemical equations that need to be balanced using the method of ionic half-reactions. It provides the chemical formulas and oxidation numbers for each element in each equation to allow for balancing the equations.
IB Chemistry on Born Haber Cycle and Lattice EnthalpyLawrence kok
The document provides information on the Born-Haber cycle and how it can be used to calculate lattice enthalpy for various ionic compounds. It gives step-by-step explanations of standard enthalpy changes used in the Born-Haber cycle calculations for ionic compounds such as LiCl, NaCl, KCl, NaBr, NaF and NaH. Diagrams illustrate the multi-stage process of determining lattice enthalpy values that cannot be measured directly through experimentation.
IB Chemistry on Born Haber Cycle and Lattice EnthalpyLawrence kok
The document describes the Born-Haber cycle process for determining the lattice enthalpy of various ionic compounds such as LiCl, NaCl, KCl, NaBr, NaF, and NaH. The Born-Haber cycle involves breaking down the ionic compound into gaseous ions and then measuring the standard enthalpy changes associated with steps such as atomization, ionization, and electron affinity which are used to calculate the unknown lattice enthalpy value. Diagrams of the Born-Haber cycle are provided for each example compound.
Periodic Table of Elements (Update) by Malik XufyanMalik Xufyan
The document provides a periodic table of the elements with the following information for each element:
1) Atomic number and common ions formed
2) Atomic symbol
3) English element name
4) Atomic mass (rounded)
The periodic table is organized into blocks by orbital type and periods by proton number. Common polyatomic ions are also listed at the bottom with their charge.
Stoichiometry is the quantitative relationship between reactants and products in chemical reactions. Hess's law states that the enthalpy change of a reaction is independent of the pathway and depends only on the initial and final states. Using Hess's law, one can determine the enthalpy change of a reaction by adding the enthalpy changes of multiple steps that combine to give the overall reaction. The standard enthalpy of formation of a compound is the enthalpy change when one mole of the substance is formed from its elements in their standard states.
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.
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 contains 10 chemical equations that need to be balanced using the method of ionic half-reactions. It provides the chemical formulas and oxidation numbers for each element in each equation to allow for balancing the equations.
IIT-JEE Mains 2017 Online Chemistry Previous Paper Day 1Eneutron
1. The document contains 10 multiple choice questions related to chemistry.
2. The questions cover topics like properties of gases, thermochemistry, electrochemistry, and freezing point depression.
3. Answer options in the form of calculations and statements related to the concepts above are provided for each question.
IB Chemistry on Hess's Law, Enthalpy Formation and CombustionLawrence kok
1) Hess's law states that the enthalpy change of a reaction is independent of the pathway and is equal to the sum of the enthalpy changes of the steps.
2) Standard enthalpy changes of formation (ΔHf°) can be used to calculate the enthalpy change (ΔH°) of a reaction by adding the standard enthalpies of formation of products and subtracting the standard enthalpies of formation of reactants.
3) For the reaction 2H2S + SO2 → 3S + 2H2O, the calculated standard enthalpy change is -234 kJ/mol.
(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.
IIT JEE 2011 Solved Paper by Prabhat GauravSahil Gaurav
(1) The document provides instructions for a test paper containing 69 multiple choice questions across 3 subjects (Chemistry, Physics, and Mathematics) divided into 4 sections each.
(2) It details the marking scheme for each section - for sections with single correct answers, marks are awarded based on selecting the right option and penalizing for wrong ones; sections with multiple correct options award marks only for fully correct responses.
(3) Instructions are given on filling details on the answer sheet correctly and handling the paper and materials during the exam.
The document describes the format and marking scheme of the IIT-JEE 2009 paper 1 exam. It includes 4 sections with different question types. Section I has 8 multiple choice questions with a single correct answer. Section II has 4 multiple choice questions where one or more answers may be correct. Section III has 2 groups of 3 questions each based on paragraphs. Section IV has 2 questions matching statements between two columns. The marking scheme awards marks for correct answers and deducts marks for incorrect answers depending on the section.
IB Chemistry on Hess's Law, Enthalpy Formation and CombustionLawrence kok
The document provides information on Hess's law and how to use standard enthalpy of formation values to calculate enthalpy changes for chemical reactions. It explains that Hess's law states that the enthalpy change for a reaction is independent of pathway and is equal to the sum of enthalpy changes in the stepwise reactions. Standard enthalpy of formation values are given for many substances, and these can be used together with Hess's law to calculate the enthalpy change of a reaction from the standard enthalpies of formation of the products and reactants. Several examples are shown of using this approach to determine enthalpy changes for different reactions.
IB Chemistry on Bond Enthalpy, Enthalpy formation, combustion and atomizationLawrence kok
This document discusses several methods to calculate enthalpy change (ΔH) for chemical reactions, including using average bond enthalpies, standard enthalpies of formation (ΔHf), standard enthalpies of combustion (ΔHc), and standard enthalpies of atomization (ΔHa). It provides examples of calculating ΔH for reactions involving CH4, CCl4, S8, carbon polymorphs, and the formation of C5H5N from carbon, hydrogen, and nitrogen. The document emphasizes that while average bond enthalpies can be used, ΔHf, ΔHc, and ΔHa are generally more accurate as they consider the specific bonds in the reaction.
1) A chemical reaction can be differentiated from a phase change or nuclear change based on whether it involves a change in chemical composition, state of matter, or type of element.
2) In a chemical reaction, reactants yield products through the rearrangement of atoms. Chemical equations use symbols to represent the reactants and products.
3) Evidence that a chemical reaction occurred includes the release or absorption of energy, production of a gas, formation of a precipitate, or a color change.
for video go my YouTube channel science world
copy this link https://youtu.be/cKbQvOxtNbI and search in youtube
In this video we solve coordination quiz part 2
#inorganicChemistry
#CoordinationChemistry
#coordinationIsomers
#crystal_field_theory
#jahn_teller_distortion
#colour_theory
#coordination_Isomers
#spin_selection_rule
#coordination_quiz
#spinalcompound
#CFT
#inverse_spinal
#normal_spinal
#JTD
#hydration_energy
#colour_of_complex_compound
#crystal_field_diagram_of_octahedral_comples
#existence_of_Ag3+
#spinal
#quiz_dicussion
#inorganicChemistry
#CoordinationChemistry
tetrahedral complex
#hydrationenergy
#NiCO4
#OsO4
#NiCl4]2-
#metal_ion
link or playlist of crystal field theory
https://youtube.com/playlist?list=PLA1jCLnc0NdOm-zSIlEtyh067DSe6sOYX
link of playlist of main group compound
https://youtube.com/playlist?list=PLA1jCLnc0NdM5yfM3IwaSy65-drs307Kq
link of hydration energy of d block element
https://youtu.be/ULaE3qwT8tQ
link of concept of hydration energy
https://youtu.be/iJ9uGR6RkeA
https://youtu.be/fB2muVLc_0A
this video very useful for all #chemistry related exam like
#jee main+ #adwance
#bsc
#msc
#iit #jam
#CSIR
#gate
#du
#bhu
#hcu
link of playlist of crystal field theory
https://youtube.com/playlist?list=PLA1jCLnc0NdOm-zSIlEtyh067DSe6sOYX
link of playlist of color theory
https://youtube.com/playlist?list=PLA1jCLnc0NdOTROKOS0axGBQn0MkkVr9d
Types of Reactions: Double Replacement and Combustionalchemist
This document discusses the five main types of chemical equations: synthesis, decomposition, single replacement, double replacement, and combustion. It provides examples of each type of equation and guides the reader through writing balanced equations for double replacement and combustion reactions. Key details include identifying the reactants and products for each reaction type, and using systematic steps to derive balanced chemical equations.
1. Serine is an amino acid with the molecular formula C3H7NO3. It consists of 3 oxygen atoms, 7 hydrogen atoms, 1 nitrogen atom, and 3 carbon atoms.
2. Molecular modeling of serine shows its 3D ball and stick structure and 5 lone electron pairs. MM2 minimization was performed to optimize the structure.
3. Key properties of serine were calculated including bond lengths, bond energies, van der Waals interactions between atoms, and angles between atom pairs. This provides important information about serine's molecular structure and interactions.
The document discusses three tables that provide standard reduction potentials (E° values) for various electrochemical reactions. Table 1 lists elements alphabetically by symbol. Table 2 lists reactions with positive E° values relative to the standard hydrogen electrode, in order of increasing potential. Table 3 lists reactions with negative E° values relative to the standard hydrogen electrode, in order of decreasing potential. The document notes some reactions have more reliable E° values than others based on number of significant figures.
IB Chemistry on Bond Enthalpy and Bond Dissociation EnergyLawrence kok
The document discusses bond enthalpy (BE) and bond dissociation energy (BDE) in calculating heat of reactions (ΔHrxn). It provides average BE values for breaking C-H (414 kJ/mol) and C-CI (325 kJ/mol) bonds. BE is an approximation of the energy needed to break a bond in the gaseous state, while BDE is the actual energy. Examples show using average BE and standard heat of formation (ΔHf°) values to determine ΔHrxn through Hess's law. More accurate methods involve determining ΔHf° or heat of combustion (ΔHc°) of reactants and products.
This document is a periodic table of elements sorted by atomic number. It lists each element's atomic number, symbol, name, atomic weight, electron configuration, and other properties. The table can be sorted by different columns such as symbol or atomic weight. It includes all 118 elements that have been discovered as of 2022.
This document provides a table of standard enthalpies of formation (ΔHformation) in kJ/mol for various common substances. It notes that Hess's law can be used to calculate the standard enthalpy of a reaction (ΔHrx) from the standard enthalpies of formation of the products and reactants. The table lists the ΔHformation values for over 30 different elements and compounds.
1. The document discusses various chemical reactions and processes involved in the production of fertilizers and other chemicals.
2. Key reactions include the contact process for producing ammonia and the Haber process for producing nitric acid. Sulfuric acid is also discussed as a key input.
3. Methods of blending fertilizers are described including bulk blending, granulation, and using various additives to improve properties of the fertilizer.
1. The document discusses various topics related to biology such as the development of blood vessels, respiration, cell organelles, and meiosis.
2. Key points include the formation of blood vessels from different germ layers, the role of hemoglobin in transporting gases, and the process of cellular respiration utilizing oxygen.
3. Various biological structures and processes are defined such as organelles, mitosis, meiosis, and the nitrogen cycle. Comparisons are made between plant and animal cells and between different types of reproduction.
This document discusses a new restaurant concept that incorporates a digital landscape and uses smartphones to enhance the dining experience. Customers would use their phones to access the menu, place orders, pay bills, and interact with digital elements in the surrounding landscape. The goal is to modernize the traditional restaurant experience through innovative technology integration.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
The Daily 5 and C.A.F.E. are literacy frameworks based on research showing the best practices for instruction. They allow teachers to differentiate instruction through small group and individual conferences while students work independently through a choice of literacy tasks. C.A.F.E. further supports literacy development by integrating reading and writing assessments to set student goals and form strategy groups in comprehension, accuracy, fluency, and expanding vocabulary.
The document discusses the results of a study on the effects of a new drug on memory and cognitive function in older adults. The double-blind study involved 100 participants aged 65-80 who were given either the drug or a placebo daily for 6 months. Researchers found that those who received the drug performed significantly better on memory and problem-solving tests at the end of the study compared to those who received the placebo.
IIT-JEE Mains 2017 Online Chemistry Previous Paper Day 1Eneutron
1. The document contains 10 multiple choice questions related to chemistry.
2. The questions cover topics like properties of gases, thermochemistry, electrochemistry, and freezing point depression.
3. Answer options in the form of calculations and statements related to the concepts above are provided for each question.
IB Chemistry on Hess's Law, Enthalpy Formation and CombustionLawrence kok
1) Hess's law states that the enthalpy change of a reaction is independent of the pathway and is equal to the sum of the enthalpy changes of the steps.
2) Standard enthalpy changes of formation (ΔHf°) can be used to calculate the enthalpy change (ΔH°) of a reaction by adding the standard enthalpies of formation of products and subtracting the standard enthalpies of formation of reactants.
3) For the reaction 2H2S + SO2 → 3S + 2H2O, the calculated standard enthalpy change is -234 kJ/mol.
(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.
IIT JEE 2011 Solved Paper by Prabhat GauravSahil Gaurav
(1) The document provides instructions for a test paper containing 69 multiple choice questions across 3 subjects (Chemistry, Physics, and Mathematics) divided into 4 sections each.
(2) It details the marking scheme for each section - for sections with single correct answers, marks are awarded based on selecting the right option and penalizing for wrong ones; sections with multiple correct options award marks only for fully correct responses.
(3) Instructions are given on filling details on the answer sheet correctly and handling the paper and materials during the exam.
The document describes the format and marking scheme of the IIT-JEE 2009 paper 1 exam. It includes 4 sections with different question types. Section I has 8 multiple choice questions with a single correct answer. Section II has 4 multiple choice questions where one or more answers may be correct. Section III has 2 groups of 3 questions each based on paragraphs. Section IV has 2 questions matching statements between two columns. The marking scheme awards marks for correct answers and deducts marks for incorrect answers depending on the section.
IB Chemistry on Hess's Law, Enthalpy Formation and CombustionLawrence kok
The document provides information on Hess's law and how to use standard enthalpy of formation values to calculate enthalpy changes for chemical reactions. It explains that Hess's law states that the enthalpy change for a reaction is independent of pathway and is equal to the sum of enthalpy changes in the stepwise reactions. Standard enthalpy of formation values are given for many substances, and these can be used together with Hess's law to calculate the enthalpy change of a reaction from the standard enthalpies of formation of the products and reactants. Several examples are shown of using this approach to determine enthalpy changes for different reactions.
IB Chemistry on Bond Enthalpy, Enthalpy formation, combustion and atomizationLawrence kok
This document discusses several methods to calculate enthalpy change (ΔH) for chemical reactions, including using average bond enthalpies, standard enthalpies of formation (ΔHf), standard enthalpies of combustion (ΔHc), and standard enthalpies of atomization (ΔHa). It provides examples of calculating ΔH for reactions involving CH4, CCl4, S8, carbon polymorphs, and the formation of C5H5N from carbon, hydrogen, and nitrogen. The document emphasizes that while average bond enthalpies can be used, ΔHf, ΔHc, and ΔHa are generally more accurate as they consider the specific bonds in the reaction.
1) A chemical reaction can be differentiated from a phase change or nuclear change based on whether it involves a change in chemical composition, state of matter, or type of element.
2) In a chemical reaction, reactants yield products through the rearrangement of atoms. Chemical equations use symbols to represent the reactants and products.
3) Evidence that a chemical reaction occurred includes the release or absorption of energy, production of a gas, formation of a precipitate, or a color change.
for video go my YouTube channel science world
copy this link https://youtu.be/cKbQvOxtNbI and search in youtube
In this video we solve coordination quiz part 2
#inorganicChemistry
#CoordinationChemistry
#coordinationIsomers
#crystal_field_theory
#jahn_teller_distortion
#colour_theory
#coordination_Isomers
#spin_selection_rule
#coordination_quiz
#spinalcompound
#CFT
#inverse_spinal
#normal_spinal
#JTD
#hydration_energy
#colour_of_complex_compound
#crystal_field_diagram_of_octahedral_comples
#existence_of_Ag3+
#spinal
#quiz_dicussion
#inorganicChemistry
#CoordinationChemistry
tetrahedral complex
#hydrationenergy
#NiCO4
#OsO4
#NiCl4]2-
#metal_ion
link or playlist of crystal field theory
https://youtube.com/playlist?list=PLA1jCLnc0NdOm-zSIlEtyh067DSe6sOYX
link of playlist of main group compound
https://youtube.com/playlist?list=PLA1jCLnc0NdM5yfM3IwaSy65-drs307Kq
link of hydration energy of d block element
https://youtu.be/ULaE3qwT8tQ
link of concept of hydration energy
https://youtu.be/iJ9uGR6RkeA
https://youtu.be/fB2muVLc_0A
this video very useful for all #chemistry related exam like
#jee main+ #adwance
#bsc
#msc
#iit #jam
#CSIR
#gate
#du
#bhu
#hcu
link of playlist of crystal field theory
https://youtube.com/playlist?list=PLA1jCLnc0NdOm-zSIlEtyh067DSe6sOYX
link of playlist of color theory
https://youtube.com/playlist?list=PLA1jCLnc0NdOTROKOS0axGBQn0MkkVr9d
Types of Reactions: Double Replacement and Combustionalchemist
This document discusses the five main types of chemical equations: synthesis, decomposition, single replacement, double replacement, and combustion. It provides examples of each type of equation and guides the reader through writing balanced equations for double replacement and combustion reactions. Key details include identifying the reactants and products for each reaction type, and using systematic steps to derive balanced chemical equations.
1. Serine is an amino acid with the molecular formula C3H7NO3. It consists of 3 oxygen atoms, 7 hydrogen atoms, 1 nitrogen atom, and 3 carbon atoms.
2. Molecular modeling of serine shows its 3D ball and stick structure and 5 lone electron pairs. MM2 minimization was performed to optimize the structure.
3. Key properties of serine were calculated including bond lengths, bond energies, van der Waals interactions between atoms, and angles between atom pairs. This provides important information about serine's molecular structure and interactions.
The document discusses three tables that provide standard reduction potentials (E° values) for various electrochemical reactions. Table 1 lists elements alphabetically by symbol. Table 2 lists reactions with positive E° values relative to the standard hydrogen electrode, in order of increasing potential. Table 3 lists reactions with negative E° values relative to the standard hydrogen electrode, in order of decreasing potential. The document notes some reactions have more reliable E° values than others based on number of significant figures.
IB Chemistry on Bond Enthalpy and Bond Dissociation EnergyLawrence kok
The document discusses bond enthalpy (BE) and bond dissociation energy (BDE) in calculating heat of reactions (ΔHrxn). It provides average BE values for breaking C-H (414 kJ/mol) and C-CI (325 kJ/mol) bonds. BE is an approximation of the energy needed to break a bond in the gaseous state, while BDE is the actual energy. Examples show using average BE and standard heat of formation (ΔHf°) values to determine ΔHrxn through Hess's law. More accurate methods involve determining ΔHf° or heat of combustion (ΔHc°) of reactants and products.
This document is a periodic table of elements sorted by atomic number. It lists each element's atomic number, symbol, name, atomic weight, electron configuration, and other properties. The table can be sorted by different columns such as symbol or atomic weight. It includes all 118 elements that have been discovered as of 2022.
This document provides a table of standard enthalpies of formation (ΔHformation) in kJ/mol for various common substances. It notes that Hess's law can be used to calculate the standard enthalpy of a reaction (ΔHrx) from the standard enthalpies of formation of the products and reactants. The table lists the ΔHformation values for over 30 different elements and compounds.
1. The document discusses various chemical reactions and processes involved in the production of fertilizers and other chemicals.
2. Key reactions include the contact process for producing ammonia and the Haber process for producing nitric acid. Sulfuric acid is also discussed as a key input.
3. Methods of blending fertilizers are described including bulk blending, granulation, and using various additives to improve properties of the fertilizer.
1. The document discusses various topics related to biology such as the development of blood vessels, respiration, cell organelles, and meiosis.
2. Key points include the formation of blood vessels from different germ layers, the role of hemoglobin in transporting gases, and the process of cellular respiration utilizing oxygen.
3. Various biological structures and processes are defined such as organelles, mitosis, meiosis, and the nitrogen cycle. Comparisons are made between plant and animal cells and between different types of reproduction.
This document discusses a new restaurant concept that incorporates a digital landscape and uses smartphones to enhance the dining experience. Customers would use their phones to access the menu, place orders, pay bills, and interact with digital elements in the surrounding landscape. The goal is to modernize the traditional restaurant experience through innovative technology integration.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
The Daily 5 and C.A.F.E. are literacy frameworks based on research showing the best practices for instruction. They allow teachers to differentiate instruction through small group and individual conferences while students work independently through a choice of literacy tasks. C.A.F.E. further supports literacy development by integrating reading and writing assessments to set student goals and form strategy groups in comprehension, accuracy, fluency, and expanding vocabulary.
The document discusses the results of a study on the effects of a new drug on memory and cognitive function in older adults. The double-blind study involved 100 participants aged 65-80 who were given either the drug or a placebo daily for 6 months. Researchers found that those who received the drug performed significantly better on memory and problem-solving tests at the end of the study compared to those who received the placebo.
Este documento presenta una introducción a la microbiología ambiental y la biodiversidad microbiana procariótica. Explica conceptos clave como microorganismos, microbiología ambiental, y diversidad microbiana. También proporciona detalles sobre la clasificación de microorganismos como virus, bacterias, hongos micelares y protozoarios. Finalmente, ofrece información sobre la estructura, reproducción y clasificación de virus, así como las características de rickettsias.
This document provides an overview of the simple present and present progressive tenses in English. It explains that the simple present is used for habitual actions, general truths, and permanent situations, while the present progressive expresses ongoing or temporary actions happening now. Examples are given for each tense. The grammar structures of the simple present and present progressive are reviewed. Practice exercises with answers are included to help distinguish between the two tenses.
The document discusses the results of a study on the effects of exercise on memory and thinking abilities in older adults. The study found that regular exercise can help reduce the decline in thinking abilities that often occurs with age. Older adults who exercised regularly performed better on cognitive tests and brain scans showed they had greater activity in important areas for memory and learning compared to less active peers.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
This document contains 49 multiple choice questions covering various topics in chemistry. The questions assess knowledge of topics including: chemical formulas and electron configurations; lattice energies; gas laws; enthalpy of formation; acid-base reactions; stoichiometry calculations; and organic reactions. The multiple choice options provided for each question require application of chemistry concepts to analyze and solve various problems.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help boost feelings of calmness, happiness and focus.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms for those who already suffer from conditions like depression and anxiety.
1. 92
15 F A-NET ( )
(1) 24Cr 29Cu F F
F
24Cr 29Cu
1. [Ar] 4s2
3d4
[Ar] 4s1
3d10
2. [Ar] 4s2
3d4
[Ar] 4s2
3d9
3. [Kr] 5s1
4d5
[Kr] 5s1
4d10
4. [Ar] 4s1
3d5
[Ar] 4s1
3d10
(2) F 60 2 F F F F 27
F ˈ F
1. 26 28 2. 33 33 3. 31 35 4. 32 33
(3) (Lattice energy)
1. NaCl 2. MgO 3. CaCl2 4.AlF3
(4) 6 bonding electrons
1. C2H4 2. CO2 3. H2S 4. NCl3
(5) F F F
1. C6H5NH2 2. C6H5CO2Na 3. CH3CH (OH) CH3 4. CH3CH (NH2) CO2H
(6) ˈ lattice energy XY
1. X (s) + Y(s) → XY(s) 2. X (g) + Y(g) → XY (s)
3.
+
)s(X +
−
)s(Y → XY (s) 4.
+
)g(X +
−
)g(Y → XY (s)
(7) F F
F (nm)
1. A -1 0.181
2. B +1 0.169
3. C +2 0.065
4 D +2 0.135
(8) 10 m3
ˈ 50 kPa 30 m3
ˈ 100 kPa F F
F ˈ F
1. 75 kPa 2. 87.5 kPa 3. 125 kPa 4. 150 kPa
(9) F ˈ (the enthalpy change of formation of a compound)
1. 2H2(g) + O2(g) → 2H2O(g) 2. Na(s) + Cl(g) → NaCl(s)
3. H2O(l) + NaCl(s) → NaCl (aq) 4. K(s) + Mn (s) + 2O2 (g) → KMnO4 (s)
2. 93
(10) ∆H F
(1) .CO(g) +
2
1
O2(g) → CO2(g) ∆H1 = -283 kJ.mol-1
(2) .H2(g) +
2
1
O2(g) → H2O(l) ∆H2 = -286 kJ.mol-1
(3) .CH3OH(l) +
2
3
O2(g) → CO2(g) 2H2O(l) ∆H3 = -715 kJ.mol-1
∆H CO(g) + 2H2(g) → CH3OH (l)
1. -146 kJ.mol-1
2. -140 kJ.mol-1
3. +140 kJ.mol-1
4. +146 kJ.mol-1
(11) F F ˈ
CaCl2 (aq) + 2NaOH(aq) → 2NaCl (aq) + Cd (OH)2(s)
NaOH F F 0.10 F 9.0 cm3
CdCl2 F F 1.00 F
500 cm3
F Cd (OH)2 ( Cd = 112.4, O = 16, H = 1)
1.
10002
146.40.109.0
×
××
2.
509
146.40.109.02 ×××
3.
1000
146.40.109.0 ××
4.
1000
146.40.109.02 ×××
(12) F ˈ F
1. CaCO3 (s) + 2HCl(ag) → CaCl2 (aq) + CO2 (g) + H2O (l)
2. CuS(s) + O2 (g) → Cu(s) + SO2 (g)
3. Hg(NO3)2(aq) + H2S (g) → HgS(s) + 2HNO3 (aq)
4. 2NaOH(aq) + H2SO4(aq) → Na2SO4 (aq) + 2H2O(l)
(13) I, II, III IV F
3. 94
F F
F I II III IV
1 F
2 F
3 F
4 F
(14) F ˈ F F 1 4 F F
ˈ
1. 2, 3 2. 2, 7 3. 2, 8, 2 4. 2, 8, 8, 1
(15) F 4 F F 500 cm3
ˈ F
1. A 2. B 3. C 4. D
(16) F F 25o
C (298 K) 101.3 kPa
1. 1.0 2. 1.0 3. 1.0 4. 1.0
(17) thorium chloride ˈ ThCl4 ammonium chromite ˈ NH4CrO2 F ˈ
thorium chromite
1. ThCrO2 2. Th2CrO2 3. Th (CrO2)4 4. Th (CrO2)2
(18) 69
Ga 68.9 71
Ga 70.9 F
69.7 F 69
Ga ˈ F
1.
9.689.70
9.687.69
−
−
= 0.40 2.
9.689.70
7.699.70
−
−
= 0.60
3.
7.699.70
9.68
+
= 0.49 4.
9.707.699.68
9.68
++
= 0.33
(19) papaverine F impotence F F 70.75% , 6.25% ,
4.13% 18.87% F papaverine 339.2
papaverine F
1. C20H21NO4 2. C20H11NO2 3. C20H23N2O3 4. C17H30NO5
I1 = 744 , I2 = 1457 , I3 = 7739 , I4 = 10547
4. 95
(20) F ˈ F 2, 2-dimethyl-3-elthyl hexane
1.
3
23
3223
3
CH
CHCH
CHCHCHCHCCH
CH
−−−−−
2.
33
323
3
CHCH
CHCHCCHCH
CH
−−−−
3.
3
32
323
3
CH
CHCH
CHCHCCHCH
CH
−−−−
4. CH3 CH2 CH2 CH2 CH CH2 CH2 CH2 CH3
CH3
(21) E F ˈ E2O3 F E ˈ F
1. Mg 2. Al 3. Si 4. P
(22) F
1. −216
8 O 2. F19
9 3. Na23
11 4. +327
13 Al
(23) F
+ 2Ag+
+ 2Ag(s) + 2H+
OH
OH
O
O
5. 96
1. 2. Ag+
3. 4. Ag
(24) F F 0.100 F 1.00
F F 0.100 F 1.00 F F ˈ F
1. 0.0500 mol L-1
2. 0.100 mol L-1
3. 0.150 mol L-1
4. 0.200 mol L-1
(25) F F 71.0 F F ( Cl = 35.5)
1. 24.5 273 K 101.3 kPa 2. 6.02 x 1023
3. 2 4. 2
(26) 5.0 F F 1.00 F 20 cm3
F F F ( Zn = 65)
1. 0.00 g 2. 0.65 g 3. 3.70 g 4. 4.35 g
(27) F
H OH O
H C C C
H H OH
˅ ˈ F
F
1. CH2O C3H6O3
2. CH2O (CH2O)n
3. C2H4O2(OH) C3H4O3
4. (CH2O)n CH2O
(28) F 0.25 F ˈ F
1. 0.50 2. 0.25 3. 3.01 x 1023
4. 1.51 x 1023
(29) F (allotropes)
1. 14
C 12
C 2. 1 2-
3. Fe2+
Fe3+
4. O2 O3
O
O
OH
OH
6. 97
(30) F :-
F 5.85 F F ˈ 250 F
F F F F ( Na = 23, Cl = 35.5)
1.
1000
250
58.5
5.85
2.
250
1000
58.5
5.85
3.
58.5
5.85
1000
250
4.
1000
250
5.85
58.5
(31) ʽ F
1. Cu + H2SO4 → CuSO4 + SO2 + H2O 2. Cu + 2H2SO4 → CuSO4 + SO2 + 2H2O
3. Cu + 2H2SO4 → Cu (SO4)2 + SO2 + 2H2O 4. 2Cu + H2SO4 → Cu2SO4 + SO2 + H2O
(32) F F F F 32800 Jg-1
F F kJ mol-1
F F F
( C=12)
1. 394000 2. 394 3. 32.8 4. 2.73
(33) pH = 3.0 F F F F
1. 3.0 mol L-1
2. 1.0 x 10-3
mol L-1
3. 1.0 x 10-11
mol L-1
4. 3.0 x 10-14
mol L-1
(34) F 1000 F 50.0 65o
C F
ˈ (kPa)
1. 35.69 kPa 2. 1408.6 kPa 3. 2000 kPa 4. 2005.9 kPa
(35) F ˈ (N2H4) F N2O4
F F
∆ o
fH (kJmol-1
)
H2O (l) -285
H2O (g) -242
N2H4(l) +51
N2H4(g) +95
N2O4 (l) -20
N2O4(g) +10
F ∆H0
F
1. +968 kJ 2. -968 kJ 3. +1050 kJ 4. -1050 kJ
2N2H4(l) + N2O4(l) → 3 N2(g) + 4H2O (g)
7. 98
36. F
(kJ mol-1
) 298 K
C C 348
C = C 614
C H 413
H H 436
∆ Ho
1. +124 kJ 2. -124 kJ 3. 2702 kJ 4. 2826 kJ
F F F F 37 39
F F F F F F kJ mol-1
F
Ca2+
(g) + 2Cl-
(g)
+1743 X -2249
Ca(g) 2Cl(g)
Y +192 +242
Ca(s) + Cl2(g) CaCl2(s)
-798
(37) Y
1. 2.
3. 4.
(38) CaCl2 (s) F
1. Ca(g) +
2
1
Cl2 (g) → CaCl(s) ∆H = -798 kJ 2. Ca(s) + Cl2(g) → CaCl2(s) ∆H = -2249 kJ
3. Ca(s) + Cl2(g) → CaCl2(s) ∆H = -798 kJ 4. Ca2+
(g) + 2Cl-
(g) → CaCl2(s) ∆H = -2249 kJ
(39) F F (Hess s law) ∆H X F kJ mol-1
1. -726 kJ mol-1
2. -363 kJ mol-1
3. +726 kJ mol-1
4. +242 kJ mol-1
(40) F ˈ
F F (AgCl) Ksp = 2.0 x 10-10
F F (Ag2CO3) Ksp = 8.0 x 10-12
C2H4 (g) + H2 (g) → C2H6 (g)
8. 99
F F F
1. AgCl F F Ag2CO3 2. Ag2CO3 F F AgCl
3. AgCl F F Ag2CO3 4. AgCl Ag2CO3 F F F
(41) F F F 40 F F F 0.10 F AgCl F F
1. 2 x 10-10
mol dm-3
2. 2 x 10-9
mol dm-3
3. 1.4 x 10-5
mol dm-3
4. 1.26 x 10-4
mol dm-3
(42) F ˈ
H2(g) + CO2 (g) H2O(g) + CO(g)
F (K) F 0.60 900 K F 2.0 F 2.0 F
F F 1.0 F F F F
F F 900 K ˈ F
1. 0.60 mol dm-3
2. 0.87 mol dm-3
3. 1.20 mol dm-3
4. 1.74 mol dm-3
(43) F ˈ F 0.287 ʽ
F F F F F Fe2+
F
F F F F F 0.103 F F F
F 9.84 cm3
ˈ
F F F ( H = 1, O = 16, Fe = 55.85, Mn = 55)
1. 0.28 2. 1.40 3. 14.0 4. 28.3
(44) 4 F
F ˈ F
1. HA 2. HB 3. HC 4. HD
(45) ˈ
F F
1. 24 2. 25 3. 27 4. 76
Fe2+
+ MnO4
-
+ 8H+
→ Fe3+
+ Mn2+
+ 4H2O
9. 100
(46) E
E F
1. 1 F
2. F ECl4
3. F F
4. F F F F F
F F F F 47-49
F F F 1 ˈ
(47) 5 (COMPOUND 5)
1. 1 butanol 2. butanoic acid 3. 1 bromobutane 4. 1 butene
(48) F 2 3
1. ʾ 2. F 3. F 4.
(49) F ˈ REACTION III
1. CH3CH2CH2CO2CH2CH2CH3 CH3CH2CH2COOH + CH2CH2CH2CH2OH
2. CH2CH2CH2CH2OH CH3 CH2 CH = CH2 + H2O
3. CH3CH2CH2COOH + HBr → CH3CH2CH2COOH2
+
+ Br-
4. CH3CH2CH2CH2OH + HBr → CH3CH2CH2CH2Br + H2O
2 , 8 , 4
H2SO4
Heat
H2O
H+
10. 101
(50) ˈ
F
1. 20 2. 40 3. 60 4. 80
(51) ˈ F ˈ
C6H5COOH C6H5COO-
+ H+
pH F F 0.100 F 20.0 cm3
F F F 0.200 F C F F F
cm3
1. 0.002 2. 0.01 3. 10 4. 100
(52) F F
(white powder) F F ˈ F F F F F
1. BaCl2, SrCl2, RbCl, CsCl 2. MgCl2 , CaCl2, LiCl, RbCl
3. MgCl2, BaCl2, RbCl 4. NaCl, MgCl2, BaCl2
11. 102
(53) F F F F F F
F F F F F F F F ˈ F
F F
1. ˈ F F F
2. ˈ
3. F
4. ˈ F F
(54) ˄ ˈ , F
F ˈ F F
F ˈ F ˂ F
F F F
. ˈ ˄
. ˄ ˈ Al (OH)3
. F F ˈ F
. F ˂ F
F F
1. F 2. F 3. , F 4. , ,
Al (s) | Al3+
(aq) ,OH-
(aq) | O2(g) (over graphite electrode)
F F ˈ F (salt bridge)
12. 103
(55) F
F F F
F F
1. , 2. , 3. , 4. , ,
(56) X + Y→ XY F
ˈ F
1. I 2. II 3. III 4. IV
(57) F 46 F X Y ˈ F XY ˈ F XY F X Y F
1. I 2. II 3. III 4. IV
. A A H2
. A F F F CO , F F CH3OH
. F F F
. F F F F F F F
13. 104
(58) F (Orange juice) ˈ
F 20 (mL) C F C ( H = 1,
C = 12, O = 16)
O H OH
O = C C C H
C = C CH2OH
HO OH
1. 4.6 × 10-4
mol 2. 4.6 × 10-5
mol 3. 8.1 × 10-4
mol 4. 8.1 × 10-5
mol
(59) F F
H O
HO CH2 C C
NH2 OH
(Tyrosine : Tyr)
H O
H C C
NH2 OH
(Glycine : Gly)
14. 105
F ˈ F Tyr Gly
O O
1. NH2 CH2 C NH CH C
CH2 OH
O
OH
O O
2. NH2 CH2 C O O CH2 CH - C
NH2 OH
O
3. HO O CH2 CH2 CH CH NH O C CH2 MH2
COOH
O
4. HO O CH2 CH C O
NH2 NH CH2 C
OH
(60) F ˈ F F
I II F F III IV F F
F I II III IV
1
2 F
3
4
F F
ʽ
F
(PVC)
I
III IV
II
15. 106
15 F A-NET ( )
F 1 F 4
F 2 F 3 =
2
AA 21 +
= 60
A1 + A2 = 120
p1 + n1 + p2 + n2 = 120
27 + n1 + 27 + n2 = 120
∴ n1 + n2 = 66
F F F
F 3 F 4
F 4 F 4 H H
C = C
H H
12 bonding electrons
O = C = O
4 bonding electrons
4 bonding electrons
6 bonding electrons
F 5 F 1 C6H5NH2
ˈ F F
F 6 F 4 F F F
F 7 F 3 (∆Hhyd.) F
F 8 F 2 = 10 + 30 = 40 m3
P1 = 50
40
10
× = 12.5 kPa
P2 = 100
40
30
× = 75 kPa
∴ = P1 + P2 = 12.5 + 75 = 87.5 kPa
F 9 F 4 ∆Hf F 1 25o
C
1 atm
Cl
N
Cl Cl
S
H H
NH2
16. 107
F 10 F 2
(1) .CO(g) +
2
1
O2(g) → CO2(g) ∆H1 = -283 kJ.mol-1
(2) x 2 2H2(g) + O2(g) → 2H2O(l) ∆H2 = -572 kJ.mol-1
(3) .CO2(g) + 2H2O(l) → CH3OH(l) +
2
3
O2(g) ∆H3 = +715 kJ.mol-1
(1) + (2) + (3) CO(g) + 2H2(g) → CH3OH (l)
∆H = -283 572 + 715 kJ.mol-1
= -140 kJ.mol-1
11. F 1
mol Cd (OH)2 =
2
1
mol NaOH
146.4
x
=
1000
9x0.10
x
2
1
∴ F Cd (OH)2 =
2x1000
46.49.0x0.10x1
12. 2
+2 -2 0 +4
CuS (s) + O2(g) Cu (s) + SO2(g)
F F ˈ F
13. F 1 I ˈ F
II ˈ F ˈ
III ˈ
IV ˈ F
14. F 3 F F I2 I3
F F 2
15. F 3 F pH F F F pH F
(C6H5COOH) ˈ F F
16. F 2 ˈ F ˈ (monatomic molecule)
1 F F
17. F 3 Th4+
+ CrO2 ˂ ˈ F Th (CrO2)4
17. 108
18. F 2 F 69
Ga
=
9.689.70
7.699.70
−
−
= 0.60
19. F 1 C20H21NO4 = (12x20)+(1x21)+(1x14)+(4x16) = 339
F F F 339.2
20. F 4 F F F F
CH3
CH3 C CH CH2 CH2 CH3
CH3 CH2CH3
2,2- dimethyl 3 ethyl hexane ˈ F F 4
21. F 2 E ˈ Al F Al2O3 E2O3
F
22. F 2 1.
−216
8 O = 8+2 = 10
2. F19
9 = 9
3. Na23
11 = 11
4.
+327
13 Al = 13 3 = 10
23. F 2 Ag+
+ e-
Ag
24. F 3 KNO3 = 0.100 x 1 = 0.100 mol ∴
−
3NO = 0.100 mol
Ca(NO3)2 = 0.100 x 1 = 0.100 mol ∴
−
3NO = 2 x 0.100 = 0.200 mol
[ ]−
3NO = 1
mol.L0.150
2
0.300
2
0.2000.100 −
==
+
25. F 3 1 mol Cl2
= 2 mol Cl
= 2 x 6.02 x 1023
= 22.4 dm3
at STP
= 2 x 35.5 g
= 71 g
26. F 4 Zn + 2HCl ZnCl2 + H2
mol Zn =
2
1
mol HCl
1000
20x1
x
2
1
65
x
=
∴ x = 0.65 g Zn = 5.00 0.65 g = 4.35 g
27. F 1 C3H6O3
ˈ F F CH2O
18. 109
28. F 3 1 mol CaCl2 F = 2 mol Cl
= 2 x 6.02 x 1023
0.25 mol CaCl2 F = 0.25x2x6.02x1023
= 3.01 x 1023
29. F 4 O2 O3 ˈ
30. F 1 [NaCl] =
ˈ
NaCl
=
1000
250
58.5
5.85
F
31. 2 ˈ F F F F
Cu + 2H2SO4 CuSO4 + SO2 + 2H2O
32. F 20 F F F F kJ, mol-1
= 1
kJ.mol
1000
32800x12 −
= 393.6 kJ.mol-1
= 394 kJ.mol-1
( )
33. F 3 pH = 3
∴ [H3O+
] = 10-pH
= 10-3
mol.dm-3
[OH-
] = 3
14
10
10
−
−
= 1.0 x 10-11
mol.dm-3
mol.L-1
34. F 4 PV = nRT = RT
M
g
.
= kPax2005.9
28.02x50
x3381000x8.134
35. F 4 ∆H0
= ∑∆ 0
fH (products) - ∑∆ 0
fH (reactants)
= [4(-242) + (3x0) [(2x51)+(-20)] kJ
= -1050kJ
36. F 2 ( )
= (1x614) + (4x413) + (1x436)
= 2702 kJ
F ( )
= (1x348) + (6x413)
= 2826 kJ
∆H0
= + 2702 2826 = -124 kJ
19. 110
37. F 1 ˈ F
38. F 3 CaCl2 (s) Ca (s) Cl2(g)
39. F 2 (2x+2249)-(192+242+1743) = 798
2x = -726
∴ x = - 363 kJ. mol-1
40. F 2 Ksp AgCl = [Ag+
]2
[Cl-
]
2.0 x 10-10
= x2
∴ x = 1.414 x 10-5
mol.dm-3
Ksp Ag2CO3 = [Ag+
] [CO3
2-
]
8x10-12
= x2
.x = x3
∴ x = 2 x10-4
mol.dm-3
Ag2 CO3 F F AgCl
41. F 2 ksp = [Ag+
] [Cl-
]
2x10-10
= (x) (0.10)
∴ k =
1.0
10x2 10−
= 2x10-9
mol.dm-3
42. F 2 K =
][CO][H
[CO]0][H
22
2
0.60 = 2
2
)x2(
x
−
∴ x = 0.87 mol.dm-3
43. F 2 5Fe2+
+ MnO4 + 8H+
5Fe2+
+Mn2+
+ 4H2O
mol MnO4 = x0.103
1000
9.84
= 1.01 x 10-3
mol
mol Fe2+
= 5 x 1.01 x 10-3
x 55.85 = 0.283 g
% Carbon = 1.40x100
0.287
0.2830.287
=
−
44. F 2 HB H+
F ˈ F
45. F 1 F peak F 24
46. F 2 E ˈ F 4A 3 F F
ˈ E4+
+ Cl-
= ECl4
47. F 4 F 1 butyl butanoate 2
1 butanol 3 butanoic acid 4 1 bromobutane
5 1 butene
48. F 3 F F F F
49. F 4 2 ˈ F (ROH) HBr F RBr + H2O
50. F 4 F F 800
C
20. 111
51. F 3 C6H5COOH + NaOH C6H5 COONa + H2O
C1V1 = C2V2
0.10 x 20 = 0.20 x V2
∴ V2 = 3
cm10
0.20
0.10x20
=
52. F 3 F Mg, Ba Rb
F ˈ MgCl2, BaCl2 RbCl
53. F 3 ˈ F F
54. F 4 F F ˈ F F
55. F 3 F ( ), ( ) ( ) F F ( ) ˈ F F F
56. F 4 IV F F F F F
57. F 2 II F F F F F
58. F 2 F 200 C
= mot
176
81x10 3−
∴ F 20
C = molx10
176
81
x
200
20 3−
= 4.6 x 10-5
mol
59. F 4
HO - CH2 CH C OH+H NH CH2 C OH F F F 4
NH2
60. F 3 I ˈ n CH2 = CH2 [-CH2-CH2]n
II ˈ n CH2 = CH [-CH2-CH]n
III C2H4 + H2O C2H5OH
IV C2H5OH + O2 CH3COOH + H2O
Cl
O
O O
Cl