Exercises number of moles
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The document provides 11 practice problems for calculating the number of moles in various chemical compounds. It lists the mass of common chemicals such as NaCl, CaCO3, HNO3, and asks the user to calculate the number of moles. It also includes more complex questions involving the mole ratios of elements within compounds, such as calculating the number of moles of oxygen in glucose or nitrogen in ammonium nitrite.
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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.
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5) Calculating theoretical and percent yields of a reaction.
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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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1) Determining empirical formulas from elemental compositions.
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5) Calculating theoretical and percent yields of a reaction.
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1) Empirical and molecular formulas, and how to determine them from elemental composition and molar mass data.
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This document contains 7 problems related to general chemistry. It provides chemical equations to balance, asks students to calculate formula weights and percent compositions of substances, defines key concepts like moles and molar mass, and has multi-step calculations involving moles, molar mass, and grams. The problems cover topics like stoichiometry, formula weights, percent composition, gas laws, and molar conversions.
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1. 18.9 grams of K2Cr2O7 are present in 50.0 mL of 0.360 M K2Cr2O7 solution.
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2. The document then provides 21 practice problems calculating things like the number of moles or grams of various substances, the molarity of different solutions, and multi-step dilution problems.
3. Students are asked to use the concepts of moles, molar mass, and molarity to solve quantitative chemistry problems involving substances in solutions.
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Limiting reactants
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Ejercicios calculo del numero de moles
Ejercicios para practicar el cálculo del número de moles. Las soluciones las podeis solicitar gratuitamente a quimicaparatodosymas@gmail.com
Soluciones al ejercicio del cálculo del número de moles
Hace unos días publicamos algunos ejercicios para calcular el número de moles (http://www.slideshare.net/quimicaparatodosymas/ejercicios-calculo-del-numero-de-moles). Espero que hayais practicado un poco; aquí teneis las soluciones razonadas. Para más información http://quimicaparatodosymuchomas.blogspot.com.es/
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This document contains 7 problems related to general chemistry. It provides chemical equations to balance, asks students to calculate formula weights and percent compositions of substances, defines key concepts like moles and molar mass, and has multi-step calculations involving moles, molar mass, and grams. The problems cover topics like stoichiometry, formula weights, percent composition, gas laws, and molar conversions.
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Stoichiometry is the study of quantitative relationships between reactants and products in a chemical reaction based on the law of conservation of mass. It can be used to calculate the amounts of substances involved in a reaction using mole ratios from a balanced chemical equation and molar masses. Specifically, stoichiometric calculations can be done between moles, between moles and mass, or between masses.
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This document defines key chemistry concepts and provides examples of their application in chemical reactions:
1. It defines combination, decomposition, and combustion reactions.
2. It defines limiting reactant, theoretical yield, and percent yield in chemical reactions.
3. It provides an example of the fermentation of glucose producing ethanol and carbon dioxide, and calculates related quantities.
4. It explains that the amount of products formed is determined by the limiting reactant being completely used up.
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To find the molar mass of an element, look up its atomic mass on the periodic table. For compounds, add up the molar masses of each element present according to the chemical formula, multiplying by the subscript if there is one. For example, the molar mass of NaCl is 58.5 g/mol, calculated from the molar masses of one Na atom and one Cl atom.
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The document outlines rules for counting atoms in chemical formulas:
1) Subscripts refer only to the atom behind them, coefficients apply to the entire compound.
2) If elements are inside parentheses, the subscript behind applies to everything inside.
3) Examples are provided to demonstrate how to use the rules to count atoms in different chemical formulas.
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This document provides an introduction to stoichiometry and calculations involving moles. It defines key terms like relative atomic mass, molar mass, mole, and Avogadro's constant. It presents methods for converting between mass and moles using molar mass. Examples demonstrate calculating moles from mass and mass from moles for various compounds. The document also shows reacting mass calculations involving moles.
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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.
#19 key
1. 18.9 grams of K2Cr2O7 are present in 50.0 mL of 0.360 M K2Cr2O7 solution.
2. The molarity of the (NH4)2SO4 solution formed from dissolving 4.28 grams of (NH4)2SO4 in 300 mL of water is 0.108 M.
3. 58.7 mL of 0.240M CuSO4 solution contains 2.25 grams of CuSO4 solute.
Counting Atoms 2a
This document provides instructions on writing chemical formulas and counting atoms in compounds. It explains that capital letters are used for elemental symbols, subscripts indicate the number of atoms, and numbers distributed throughout a compound indicate how many of each atom are present. Examples are given for common compounds and ions to demonstrate how to count the total number of each type of atom.
Moles
The document discusses moles, which are a unit used to measure very large quantities in chemistry. A mole is defined as 6.02 x 1023 particles, such as atoms, molecules, ions. This number is known as Avogadro's number. The document provides examples of how many everyday items would equal a mole to demonstrate just how large a mole is. It also discusses how moles can be used to convert between the number of particles, moles, and mass in grams.
Chemical reactions and stoichiometry
Triethylene glycol.
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1. The document discusses moles, molar mass, molarity, and provides example calculations involving these concepts. Molarity is defined as the number of moles of solute per liter of solution.
2. The document then provides 21 practice problems calculating things like the number of moles or grams of various substances, the molarity of different solutions, and multi-step dilution problems.
3. Students are asked to use the concepts of moles, molar mass, and molarity to solve quantitative chemistry problems involving substances in solutions.
The Mole 9.5
The document provides examples for calculating percentage composition by mass of elements in compounds. It gives the formula for finding percentage composition and worked examples calculating the percentage of elements like nitrogen and hydrogen in ammonia, hydrogen and oxygen in hydrogen peroxide, and water in copper(II) sulfate and iron(III) chloride hexahydrate.
Stoichiometry
The document discusses chemical reactions and stoichiometry. It defines stoichiometry as using ratios to determine quantities of reactants and products in a chemical reaction. It explains that coefficients in a balanced chemical equation represent molar ratios and can be used to determine moles, mass, and volume of substances in a reaction. It provides examples of solving stoichiometry problems, including determining limiting reactants.
Counting Atoms
The document provides rules for counting atoms in chemical formulas including: using subscripts only for the atom behind it, multiplying coefficients and subscripts, and applying subscripts inside parentheses to all elements within. It then provides examples of using the rules to determine the number of each type of atom in sample formulas.
Limiting reactants
This document provides examples of how to calculate the limiting reactant and maximum product formed in chemical reactions. It demonstrates calculating moles of each reactant, comparing reactant ratios to determine the limiting reactant, and using mole ratios to calculate maximum product. An alternative method is proposed to systematically solve these types of problems.
Stoichiometry & The Mole
Class presentation for our Mole and Stoichiometry units as part of the Grade 9 Introduction to Chemistry course.
Counting atoms
This document provides rules for counting atoms in chemical formulas:
1) Subscripts refer only to the atom behind them. Coefficients multiply the entire formula.
2) Subscripts inside parentheses apply to everything within.
3) Examples are provided to demonstrate how to count atoms in different chemical formulas using these rules.
Counting atoms
This document outlines the 4 rules for counting atoms in chemical compounds:
1) Element symbols represent single atoms, 2) Subscripts indicate the number of atoms, 3) Subscripts outside brackets multiply all elements inside, and 4) Coefficients multiply the total number of atoms in the formula unit. Examples are given to demonstrate how to use the rules to count the total number of each type of atom in various compounds like Mg3(PO4)2, H2O, and CH3CH2OH. The document concludes with challenges to build molecular models and count atoms in additional compounds.
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- 1. 2013 Exercises for practising the calculation of the number of moles http://quimicaparatodosymuchomas.blogspot.com.es/ 14/03/2013
- 2. Calculate the number of moles of the following molecules: 1.- 35 g of NaCl 2.- 50 g of CaCO3 3.- 100 mg of HNO3 4.- 36 g of H3PO4 5.- 1 kg of CH3OH (methanol) 6.- 63 g of SnCl4 7.- 89 g of C12H22O11 (sucralose) 8.- 390 g of CON2H4 (urea) 9.- How many moles of oxygen are there in 3 moles of C6H12O6 (glucose)? 10.- ¿How many moles of nitrogen (N) are there in 3.5 g of NH4NO2 (ammonium nitrite)? 11.- ¿How many moles of the nitrite ion (NO2-) are there in 3.5 gramos of NH4NO2 (ammonium nitrite)? You can ask for the solutions of this exercise free of charge at quimicaparatodosymas@gmail.com.