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Ch.3 - Mass Relationships in Chemical Reactions
Chapter 3, Problem 79

Sodium azide (NaN3) yields N2 gas when heated to 300 °C, a reaction used in automobile air bags. If 1.00 mol of N2 has a volume of 47.0 L under the reaction conditions, how many liters of gas can be formed by heating 38.5 g of NaN3? The reaction is

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this case, understanding the stoichiometric coefficients of sodium azide and nitrogen gas will help in calculating how much N2 can be produced from a given mass of NaN3.
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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For sodium azide (NaN3), calculating its molar mass is essential to convert the mass of NaN3 (38.5 g) into moles. This conversion is necessary to apply stoichiometry and determine the volume of nitrogen gas produced from the decomposition of sodium azide.
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Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law allows us to calculate the volume of gas produced under specific conditions. In this scenario, knowing that 1.00 mol of N2 occupies 47.0 L at the given temperature enables us to find the volume of nitrogen gas generated from the moles of NaN3 decomposed.
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Related Practice
Textbook Question

How many grams of each product result from the following reactions, and how many grams of which reactant is left over? (a)

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Textbook Question

How many grams of each product result from the following reactions, and how many grams of which reactant is left over? (b)

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Textbook Question

Limestone (CaCO3) reacts with hydrochloric acid according to the equation CaCO3 + 2 HCl ---> CaCl2 + H2O + CO2. If 1.00 mol of CO2 has a volume of 22.4 L under the reaction conditions, how many liters of gas can be formed by reaction of 2.35 g of CaCO3 with 2.35 g of HCl? Which reactant is limiting?

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Textbook Question
Acetic acid (CH3CO2H) reacts with isopentyl alcohol (C5H12O) to yield isopentyl acetate (C7H14O2), a fragrant substance with the odor of bananas. If the yield from the reaction of acetic acid with isopentyl alcohol is 45%, how many grams of isopentyl acetate are formed from 3.58 g of acetic acid and 4.75 g of isopentyl alcohol? The reaction is CH3CO2H + C5H12O ---> C7H14O2 + H2O
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Textbook Question
Cisplatin [Pt(NH3)2Cl2], a compound used in cancer treat-ment, is prepared by reaction of ammonia with potassium tetrachloroplatinate: K2PtCl4 + 2 NH3 ----> 2 KCl + Pt(NH3)2Cl2 How many grams of cisplatin are formed from 55.8 g of K2PtCl4 and 35.6 g of NH3 if the reaction takes place in 95% yield based on the limiting reactant?
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Textbook Question
If 1.87 g of acetic acid (CH3COOH) reacts with 2.31 g of isopentyl alcohol (C5H12O) to give 2.96 g of isopentyl acetate (C7H14O2), what is the percent yield of the reaction?
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