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Title: Quantities in Chemical Reactions STOICHIOMETRY PROBLEMS 1 Quantities in Chemical Reactions STOICHIOMETRY PROBLEMS • Section 5.4 2 What is Stoichiometry? • The study of quantitative relationships within chemical reactions • A balanced equation is the key to stoichiometry! • Tools youll need for this chapter • Writing proper formulas and balanced equations • Finding molar mass • Converting from mass to moles and vice versa 3 Balanced Reaction Equations and the Mole Ratio • Consider this balanced reaction equation • 4 Al(s) 3 O2(g)? 2 Al2O3(s) • The coefficients of this reaction represent • - the number of reacting PARTICLES or • - the number of reacting MOLES • These numbers are FIXED, the ratio of reacting substances NEVER changes. 4 Stoichiometry Problems • There are three types of stoichiometry problems we will encounter • Mole-Mole problems (1 conversion factor) • Mass-Mole problems (2 conversion factors) • Mass-Mass problems (3 conversion factors) given required 5 Mole-Mole Problems • Step 1 Write a BALANCED EQUATION • Step 2 Determine the mole ratio from the coefficients in the equation. • Mole ratio moles of required substance • moles of given substance • Step 3 Multiply the amount of moles of the given substance by the mole ratio • 6 Mole-Mole Problems Example 2 H2O 2 H2 O2 How many moles of water can be formed from 0.5 mol H2?
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2 mol H2O 0.5 mol H2 0.5 mol H2O x 2 mol H2 7 Mole-Mole Practice CuSO4 Al Al2(SO4)3 Cu How many moles of copper(II) sulfate will react with 0.5 moles of aluminum? 8 Mass-Mole Problems Example 2 H2O 2 H2 O2 How many moles of water can be formed from 48.0 g O2? 9 Setting up the given information 10 Mass-Mole Problems • Step 1 Write a BALANCED EQUATION. • Step 2 Convert the mass of your given substance to moles using molar mass. • Step 3 Determine the moles of your required substance using the mole ratio. 11 Setting up the given information Step 1 Step 2 M 32.00g/mol Step 3 12 Mass-Mole Problems Example 2 H2O 2 H2 O2 How many moles of water can be formed from 48.0 g O2?
Chapter 10 – Chemical Quantities. Section 10.1 – The Mole: A Measurement of Matter. You often measure the amount of something by count, by mass, or by volume. A mole (mol) of a substance is 6.02 x 1023representative particles of that substance. Chapter 10 Chemical Quantities Workbook Answer Syllabus bdm international best english medium school, english: a to z / a to z in phonetics and with pictures (recognition only) numbers: 1 to 20, shapes (triangle.
2 mol H2O 1 mol O2 48.0 g O2 3.00 mol H2O x x 1 mol O2 32.00 g O2 13 Mass-Mole Practice How many moles of aluminum sulphate can be produced from 13.5 g of aluminum? Mole ratio 1 mol Al2(SO4)3 1 mol Al 13.5 g Al x 0.250 mol Al2(SO4)3 x 2 mol Al 26.98 g Al 14 Mass-Mole Practice Ca AlCl3 CaCl2 Al 3 How many moles of calcium chloride will be produced if 5.7g of calcium is used up in the reaction? 15 Mass-Mole Practice Ca AlCl3 CaCl2 Al 3 How many moles of calcium chloride will be produced if 5.7g of calcium is used up in the reaction? How to install the sentricard utility and renew your. 3 mol CaCl2 1 mol Ca 5.7 g Ca x 0.14 mol CaCl2 x 3 mol Ca 40.08 g Ca 16 Mass-Mass Problems Example How many grams of water can be formed from 48.0 g O2? 17 Setting up the given information Step 1 Step 2 M 32.00g/mol Step 4 M 18.02g/mol Step 3 18 Mass-Mass Problems Example How many grams of water can be formed from 48.0 g O2?