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The document discusses molarity and calculations involving moles, molar mass, and number of particles. It provides examples of calculating the molecular masses of SO2 and caffeine based on given atomic masses. It also gives an example of calculating the number of moles in 5.68 g of iron using the formula n=mass/molar mass, finding the number of moles to be 0.1 mol.
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This document contains 6 chemistry problems dealing with gas stoichiometry and gas behavior:
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The document contains 6 chemistry problems involving gas phase chemical equilibria calculations:
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This document discusses calculating reacting masses in chemical reactions from balanced chemical equations. It provides examples of calculating the mass of products formed given the mass of reactants or vice versa. The key steps are: 1) calculating moles of reactants, 2) using the mole ratio from the balanced equation to determine moles of products, 3) calculating mass of products from moles and molar mass. Several example calculations are shown and questions are provided for practice.
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The document discusses moles, molar mass, molar concentration, and stoichiometry. It defines a mole as 6.02 x 1023 particles, whether atoms, molecules, ions, or electrons. Molar mass is the mass of one mole of a substance in grams. Molar concentration, or molarity, expresses the moles of solute per liter of solution. Stoichiometry uses mole ratios from balanced chemical equations to calculate amounts of reactants and products.
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This document contains 6 chemistry problems dealing with gas stoichiometry and gas behavior:
1) It defines Dalton's Law of partial pressures and shows equations for calculating total and partial pressures.
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3) It calculates the partial pressures of a gas mixture given the total pressure and amounts of each gas.
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The document contains 6 chemistry problems involving gas phase chemical equilibria calculations:
1) Calculating the equilibrium partial pressure of N2O4 and the equilibrium constant Kp for the reaction N2O4 ⇌ 2NO2.
2) Calculating the equilibrium concentrations of H2, Br2, and HBr and the equilibrium constant Kc for the reaction H2 + Br2 ⇌ 2HBr.
3) Calculating the equilibrium constant Kc for the reaction SO2 + Cl2 ⇌ SO2Cl2 given the value of Kp.
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The document discusses concepts related to counting molecules and determining formula mass and molar mass. It provides examples of calculating formula mass for various compounds by identifying the elements in the chemical formula, looking up the atomic mass of each element, multiplying by the subscript if present, and summing the atomic masses. It also discusses hydrates, how to name them, and how to calculate their formula mass by including the mass of water molecules.
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The document discusses the mole concept in chemistry. Some key points:
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This document contains a chemistry lesson on molar mass. It defines molar mass as the sum of the atomic masses in a molecule. It provides examples of calculating the molar mass of different compounds by adding up the atomic masses of each element. The lesson concludes by having students practice calculating molar masses in groups and answering an exit slip with questions.
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2. The mass of one mole of a substance can be calculated from its relative atomic/molecular mass. For example, one mole of carbon has a mass of 12g while one mole of oxygen has a mass of 32g.
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The document discusses key concepts related to moles including:
1) Definitions of relative atomic mass (RAM), relative formula mass (RFM), and relative molecular mass (RMM) which refer to the average mass of atoms and molecules.
2) How to calculate RAM, RFM, and RMM using the periodic table and chemical formulas.
3) What a mole is and how it relates to Avogadro's number to allow counting and measuring very large numbers of small entities like atoms and molecules.
Simple moles
The document discusses key concepts related to moles including:
1) Definitions of relative atomic mass (RAM), relative formula mass (RFM), and relative molecular mass (RMM) which refer to the average mass of atoms and molecules.
2) How to calculate RAM, RFM, and RMM using the periodic table and chemical formulas.
3) What a mole is and how it relates to Avogadro's number to allow counting and measuring very large numbers of small entities like atoms and molecules.
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This document provides instructions for completing stoichiometry calculations using mass-to-mass conversions. It includes a sample reaction and 5 practice problems using the reaction between sulfur, oxygen, hydrogen, and sulfuric acid. The instructions emphasize converting between grams and moles in 3 steps: 1) convert mass to moles, 2) use mole ratios from the balanced chemical equation, and 3) convert moles back to mass. Work must be shown for full credit.
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Microorganisms interacts with each other and can be physically associated with another organisms in a variety of ways.
One organism can be located on the surface of another organism as an ectobiont or located within another organism as endobiont.
Microbial interaction may be positive such as mutualism, proto-cooperation, commensalism or may be negative such as parasitism, predation or competition
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Positive interaction: mutualism, proto-cooperation, commensalism
Negative interaction: Ammensalism (antagonism), parasitism, predation, competition
I. Mutualism:
It is defined as the relationship in which each organism in interaction gets benefits from association. It is an obligatory relationship in which mutualist and host are metabolically dependent on each other.
Mutualistic relationship is very specific where one member of association cannot be replaced by another species.
Mutualism require close physical contact between interacting organisms.
Relationship of mutualism allows organisms to exist in habitat that could not occupied by either species alone.
Mutualistic relationship between organisms allows them to act as a single organism.
Examples of mutualism:
i. Lichens:
Lichens are excellent example of mutualism.
They are the association of specific fungi and certain genus of algae. In lichen, fungal partner is called mycobiont and algal partner is called
II. Syntrophism:
It is an association in which the growth of one organism either depends on or improved by the substrate provided by another organism.
In syntrophism both organism in association gets benefits.
Compound A
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In this theoretical example of syntrophism, population 1 is able to utilize and metabolize compound A, forming compound B but cannot metabolize beyond compound B without co-operation of population 2. Population 2is unable to utilize compound A but it can metabolize compound B forming compound C. Then both population 1 and 2 are able to carry out metabolic reaction which leads to formation of end product that neither population could produce alone.
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Methane produced by methanogenic bacteria depends upon interspecies hydrogen transfer by other fermentative bacteria.
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The document outlines an chemistry class where students will learn about stoichiometry, mole ratios, and balancing chemical equations. Students are instructed to take notes on mole ratios and balancing equations using examples worked through in class. For homework, students are asked to finish practice problems on these topics in preparation for an upcoming exam.
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This document contains 5 examples of stoichiometry calculations involving chemical reactions. Each example provides the balanced chemical equation, the relevant atomic masses, and step-by-step working to calculate the amounts of reactants and products based on the mole ratios in the balanced equations. The examples calculate amounts of unreacted iron, masses of products formed from decomposing calcium carbonate, amounts of sodium hydroxide and water formed from a reaction of sodium hydroxide and sulfuric acid, tonnes of carbon and copper produced from a copper smelting reaction, and tonnes of carbon needed to reduce iron oxide ore.
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The document provides information on calculating relative atomic masses (Mr) and mass of products in chemical reactions. It gives the formulas to calculate Mr of compounds by adding the atomic masses of elements. It also provides methods to calculate percentage composition and mass of products using the ratio of Mr of products to reactants. Examples are given to calculate mass of MgO from Mg, H2 from H2O, CaO from Ca, and Al from Al2O3.
Moles
1. A mole is a unit used to quantify an amount of substance and refers to 6.022x10^23 elementary entities, whether atoms, molecules, ions or other particles.
2. The mass of one mole of a substance can be calculated from its relative atomic/molecular mass. For example, one mole of carbon has a mass of 12g while one mole of oxygen has a mass of 32g.
3. Moles allow for stoichiometric calculations to determine amounts of reactants and products in chemical reactions and for calculating molar concentrations in solutions.
Class XI Chemistry - Mole Concept
The document discusses the mole concept in chemistry. Some key points:
- A mole is equal to 6.022x10^23 particles and can refer to atoms, molecules, etc.
- The molar mass of an element is its atomic mass in grams and the molar mass of a compound is the sum of the atomic masses of its elements.
- One mole of an ideal gas occupies 22.4 liters at STP.
- Questions at the end calculate things like moles, mass, volume using molar mass and mole ratios in chemical equations.
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This document contains a chemistry lesson on molar mass. It defines molar mass as the sum of the atomic masses in a molecule. It provides examples of calculating the molar mass of different compounds by adding up the atomic masses of each element. The lesson concludes by having students practice calculating molar masses in groups and answering an exit slip with questions.
Moles
1. A mole is a unit used to quantify an amount of substance and refers to 6.022x10^23 elementary entities, whether atoms, molecules, ions or other particles.
2. The mass of one mole of a substance can be calculated from its relative atomic/molecular mass. For example, one mole of carbon has a mass of 12g while one mole of oxygen has a mass of 32g.
3. Moles allow for stoichiometric calculations to determine amounts of reactants and products in chemical reactions and for calculating molar concentrations in solutions.
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The document provides examples of determining empirical and molecular formulas from elemental compositions, balancing chemical equations, calculating theoretical and percent yields of chemical reactions. It includes the following examples:
1) Determining the empirical formulas K3PO4 and Na2SiF6 from elemental compositions.
2) Calculating molecular formulas of H2C2O4 and C4H8O2 given empirical formulas and molar masses.
3) Balancing the equation Fe2O3 + CO → Fe + CO2 and calculating grams of reactants and products.
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The document discusses chemical formulae and equations. It explains that the relative atomic mass (Ar) of an element is calculated as the mass of one atom of that element divided by 1/12 the mass of one carbon-12 atom. Carbon-12 was chosen as the standard because it exists as a solid at room temperature and is easily handled, though it has three isotopes. The relative molecular mass (Mr) of a molecule is calculated by adding the Ar values of each atom in the chemical formula. Examples of calculating the Mr of MgCO3 and HPO4 are provided.
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The document discusses empirical formulas, stoichiometry, percentage yield calculations, and identifying limiting reagents. It provides examples of calculating empirical formulas from elemental composition percentages. It also gives examples of finding the limiting reagent, calculating theoretical yield, and determining percentage yield in chemical reactions.
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The document discusses the mole concept and molar volume in chemistry. It defines the molar volume as the volume occupied by one mole of a gas or gas particles. It states that one mole of any gas will have the same volume under the same temperature and pressure. The molar volume of any gas at STP is 22.4 dm3/mol. At room temperature and pressure, the molar volume is 24 dm3/mol. It provides examples of calculating the number of moles and volume of gases using molar volume.
Worksheet 11 equilibrium calculations
1. The document outlines the general procedure for solving equilibrium problems which includes: tabulating initial and equilibrium concentrations, calculating concentration changes, using stoichiometry to determine other concentration changes, calculating equilibrium concentrations, and computing the equilibrium constant Keq.
2. It then provides 5 example equilibrium problems to solve using this procedure, involving reactions of ammonia dissolving in water, sulfur trioxide decomposing, calcium chromate dissolving, the Haber process of nitrogen and hydrogen reacting to form ammonia, and a general reaction of reactants A and B forming products C and D.
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This chapter discusses chemical formulae and equations. It defines relative atomic mass and relative molecular mass, and explains how to calculate these values. It also describes the mole concept and relationships between number of moles, particles, and mass or volume. It discusses writing chemical formulae for elements, compounds, ions and ionic compounds. The chapter also explains how to determine empirical and molecular formulae, and how to balance chemical equations.
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To determine the rate exponent of a reaction, experiments are conducted where the concentration of one reactant is varied while keeping other concentrations constant. This allows observation of how the reaction rate changes and determines the order of the reaction with respect to that reactant. For a second order reaction, doubling the concentration of a reactant will quadruple the reaction rate.
Simple moles
The document discusses key concepts related to moles including:
1) Definitions of relative atomic mass (RAM), relative formula mass (RFM), and relative molecular mass (RMM) which refer to the average mass of atoms and molecules.
2) How to calculate RAM, RFM, and RMM using the periodic table and chemical formulas.
3) What a mole is and how it relates to Avogadro's number to allow counting and measuring very large numbers of small entities like atoms and molecules.
Simple moles
The document discusses key concepts related to moles including:
1) Definitions of relative atomic mass (RAM), relative formula mass (RFM), and relative molecular mass (RMM) which refer to the average mass of atoms and molecules.
2) How to calculate RAM, RFM, and RMM using the periodic table and chemical formulas.
3) What a mole is and how it relates to Avogadro's number to allow counting and measuring very large numbers of small entities like atoms and molecules.
Mass to mass worksheet example
This document provides instructions for completing stoichiometry calculations using mass-to-mass conversions. It includes a sample reaction and 5 practice problems using the reaction between sulfur, oxygen, hydrogen, and sulfuric acid. The instructions emphasize converting between grams and moles in 3 steps: 1) convert mass to moles, 2) use mole ratios from the balanced chemical equation, and 3) convert moles back to mass. Work must be shown for full credit.
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Microbial interaction
Microorganisms interacts with each other and can be physically associated with another organisms in a variety of ways.
One organism can be located on the surface of another organism as an ectobiont or located within another organism as endobiont.
Microbial interaction may be positive such as mutualism, proto-cooperation, commensalism or may be negative such as parasitism, predation or competition
Types of microbial interaction
Positive interaction: mutualism, proto-cooperation, commensalism
Negative interaction: Ammensalism (antagonism), parasitism, predation, competition
I. Mutualism:
It is defined as the relationship in which each organism in interaction gets benefits from association. It is an obligatory relationship in which mutualist and host are metabolically dependent on each other.
Mutualistic relationship is very specific where one member of association cannot be replaced by another species.
Mutualism require close physical contact between interacting organisms.
Relationship of mutualism allows organisms to exist in habitat that could not occupied by either species alone.
Mutualistic relationship between organisms allows them to act as a single organism.
Examples of mutualism:
i. Lichens:
Lichens are excellent example of mutualism.
They are the association of specific fungi and certain genus of algae. In lichen, fungal partner is called mycobiont and algal partner is called
II. Syntrophism:
It is an association in which the growth of one organism either depends on or improved by the substrate provided by another organism.
In syntrophism both organism in association gets benefits.
Compound A
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Examples of syntrophism:
i. Methanogenic ecosystem in sludge digester
Methane produced by methanogenic bacteria depends upon interspecies hydrogen transfer by other fermentative bacteria.
Anaerobic fermentative bacteria generate CO2 and H2 utilizing carbohydrates which is then utilized by methanogenic bacteria (Methanobacter) to produce methane.
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Isolation of pure culture, its various method.
在线办理(salfor毕业证书)索尔福德大学毕业证毕业完成信一模一样
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Discovery of An Apparent Red, High-Velocity Type Ia Supernova at 𝐳 = 2.9 wi...
We present the JWST discovery of SN 2023adsy, a transient object located in a host galaxy JADES-GS
+
53.13485
−
27.82088
with a host spectroscopic redshift of
2.903
±
0.007
. The transient was identified in deep James Webb Space Telescope (JWST)/NIRCam imaging from the JWST Advanced Deep Extragalactic Survey (JADES) program. Photometric and spectroscopic followup with NIRCam and NIRSpec, respectively, confirm the redshift and yield UV-NIR light-curve, NIR color, and spectroscopic information all consistent with a Type Ia classification. Despite its classification as a likely SN Ia, SN 2023adsy is both fairly red (
�
(
�
−
�
)
∼
0.9
) despite a host galaxy with low-extinction and has a high Ca II velocity (
19
,
000
±
2
,
000
km/s) compared to the general population of SNe Ia. While these characteristics are consistent with some Ca-rich SNe Ia, particularly SN 2016hnk, SN 2023adsy is intrinsically brighter than the low-
�
Ca-rich population. Although such an object is too red for any low-
�
cosmological sample, we apply a fiducial standardization approach to SN 2023adsy and find that the SN 2023adsy luminosity distance measurement is in excellent agreement (
≲
1
�
) with
Λ
CDM. Therefore unlike low-
�
Ca-rich SNe Ia, SN 2023adsy is standardizable and gives no indication that SN Ia standardized luminosities change significantly with redshift. A larger sample of distant SNe Ia is required to determine if SN Ia population characteristics at high-
�
truly diverge from their low-
�
counterparts, and to confirm that standardized luminosities nevertheless remain constant with redshift.
Authoring a personal GPT for your research and practice: How we created the Q...
Thematic analysis in qualitative research is a time-consuming and systematic task, typically done using teams. Team members must ground their activities on common understandings of the major concepts underlying the thematic analysis, and define criteria for its development. However, conceptual misunderstandings, equivocations, and lack of adherence to criteria are challenges to the quality and speed of this process. Given the distributed and uncertain nature of this process, we wondered if the tasks in thematic analysis could be supported by readily available artificial intelligence chatbots. Our early efforts point to potential benefits: not just saving time in the coding process but better adherence to criteria and grounding, by increasing triangulation between humans and artificial intelligence. This tutorial will provide a description and demonstration of the process we followed, as two academic researchers, to develop a custom ChatGPT to assist with qualitative coding in the thematic data analysis process of immersive learning accounts in a survey of the academic literature: QUAL-E Immersive Learning Thematic Analysis Helper. In the hands-on time, participants will try out QUAL-E and develop their ideas for their own qualitative coding ChatGPT. Participants that have the paid ChatGPT Plus subscription can create a draft of their assistants. The organizers will provide course materials and slide deck that participants will be able to utilize to continue development of their custom GPT. The paid subscription to ChatGPT Plus is not required to participate in this workshop, just for trying out personal GPTs during it.
Pests of Storage_Identification_Dr.UPR.pdf
InIndia-post-harvestlosses-unscientificstorage,insects,rodents,micro-organismsetc.,accountforabout10percentoftotalfoodgrains
Graininfestation
Directdamage
Indirectly
•theexuviae,skin,deadinsects
•theirexcretawhichmakefoodunfitforhumanconsumption
About600speciesofinsectshavebeenassociatedwithstoredgrainproducts
100speciesofinsectpestsofstoredproductscauseeconomiclosses
Immersive Learning That Works: Research Grounding and Paths Forward
We will metaverse into the essence of immersive learning, into its three dimensions and conceptual models. This approach encompasses elements from teaching methodologies to social involvement, through organizational concerns and technologies. Challenging the perception of learning as knowledge transfer, we introduce a 'Uses, Practices & Strategies' model operationalized by the 'Immersive Learning Brain' and ‘Immersion Cube’ frameworks. This approach offers a comprehensive guide through the intricacies of immersive educational experiences and spotlighting research frontiers, along the immersion dimensions of system, narrative, and agency. Our discourse extends to stakeholders beyond the academic sphere, addressing the interests of technologists, instructional designers, and policymakers. We span various contexts, from formal education to organizational transformation to the new horizon of an AI-pervasive society. This keynote aims to unite the iLRN community in a collaborative journey towards a future where immersive learning research and practice coalesce, paving the way for innovative educational research and practice landscapes.
Sexuality - Issues, Attitude and Behaviour - Applied Social Psychology - Psyc...
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
Compexometric titration/Chelatorphy titration/chelating titration
Classification
Metal ion ion indicators
Masking and demasking reagents
Estimation of Magnisium sulphate
Calcium gluconate
Complexometric Titration/ chelatometry titration/chelating titration, introduction, Types-
1.Direct Titration
2.Back Titration
3.Replacement Titration
4.Indirect Titration
Masking agent, Demasking agents
formation of complex
comparition between masking and demasking agents,
Indicators/Metal ion indicators/ Metallochromic indicators/pM indicators,
Visual Technique,PM indicators (metallochromic), Indicators of pH, Redox Indicators
Instrumental Techniques-Photometry
Potentiometry
Miscellaneous methods.
Complex titration with EDTA.
Applied Science: Thermodynamics, Laws & Methodology.pdf
When I was asked to give a companion lecture in support of ‘The Philosophy of Science’ (https://shorturl.at/4pUXz) I decided not to walk through the detail of the many methodologies in order of use. Instead, I chose to employ a long standing, and ongoing, scientific development as an exemplar. And so, I chose the ever evolving story of Thermodynamics as a scientific investigation at its best.
Conducted over a period of >200 years, Thermodynamics R&D, and application, benefitted from the highest levels of professionalism, collaboration, and technical thoroughness. New layers of application, methodology, and practice were made possible by the progressive advance of technology. In turn, this has seen measurement and modelling accuracy continually improved at a micro and macro level.
Perhaps most importantly, Thermodynamics rapidly became a primary tool in the advance of applied science/engineering/technology, spanning micro-tech, to aerospace and cosmology. I can think of no better a story to illustrate the breadth of scientific methodologies and applications at their best.
Methods of grain storage Structures in India.pdf
•Post-harvestlossesaccountforabout10%oftotalfoodgrainsduetounscientificstorage,insects,rodents,micro-organismsetc.,
•Totalfoodgrainproductioninindiais311milliontonnesandstorageis145mt.InIndia,annualstoragelosseshavebeenestimated14mtworthofRs.7,000croreinwhichinsectsaloneaccountfornearlyRs.1,300crores.
•InIndiaoutofthetotalproduction,about30%ismarketablesurplus
•Remaining70%isretainedandstoredbyfarmersforconsumption,seed,feed.Hence,growerneedstoragefacilitytoholdaportionofproducetosellwhenthemarketingpriceisfavourable
•TradersandCo-operativesatmarketcentresneedstoragestructurestoholdgrainswhenthetransportfacilityisinadequate
The cost of acquiring information by natural selection
This is a short talk that I gave at the Banff International Research Station workshop on Modeling and Theory in Population Biology. The idea is to try to understand how the burden of natural selection relates to the amount of information that selection puts into the genome.
It's based on the first part of this research paper:
The cost of information acquisition by natural selection
Ryan Seamus McGee, Olivia Kosterlitz, Artem Kaznatcheev, Benjamin Kerr, Carl T. Bergstrom
bioRxiv 2022.07.02.498577; doi: https://doi.org/10.1101/2022.07.02.498577
Summary Of transcription and Translation.pdf
Hello Everyone Here We are Sharing You with The process of protien Synthesis in very short points you will be Able to understand It Very well
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mole map
- 1. Map of molarity Mole mass solids/liquids formula for mole calculation n= mass/ molar.mass n=m/mol.m m=n*mol.mass particles n=no pf particlas/avagadros numb no of particles=n*avagadros numb gases n=vol(dm3)/22.4 dm3.mol-1 n=vol(dm3) at stp/molar vol
- 2. Practice problem 1.1 Calculate the molecular masses (in amu) of the following compounds: SO2 Caffeine (C8H10N4O2) Atomic mass of C=12, s=32, N=14, H=1, O=16 Solution: SO2 32+2(16) =64 amu Caffeine (C8H10N4O2) 8(12) +10(1) +4(14) +2(16) = 194 amu.
- 3. Practice problem 1.1 Calculate the number of moles in 5.68 g of iron. Atomic mass of iron Fe=55.8 Solution: No of moles=n=? Mass of Fe=5.68 g As we know that n= mass/ molar. Mass so by putting values in the formula n=5.68 g /55.8 g.mol -1 , n= 0.1 mol.