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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Ch.3 - Mass Relationships in Chemical Reactions
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 3, Problem 78
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?
Verified step by step guidance1
Calculate the molar mass of CaCO_3 and HCl using the periodic table: CaCO_3 = 40.08 (Ca) + 12.01 (C) + 3*16.00 (O) and HCl = 1.01 (H) + 35.45 (Cl).
Convert the mass of CaCO_3 and HCl to moles using their respective molar masses: moles = mass / molar mass.
Determine the stoichiometry of the reaction from the balanced equation: 1 mole of CaCO_3 reacts with 2 moles of HCl to produce 1 mole of CO_2.
Identify the limiting reactant by comparing the mole ratio of the reactants to the stoichiometric ratio from the balanced equation.
Calculate the volume of CO_2 produced using the moles of the limiting reactant and the given volume of 1 mole of CO_2 (22.4 L/mol).
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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 based on the balanced chemical equation. It allows us to determine the amount of product formed or reactant consumed by using mole ratios derived from the coefficients in the balanced equation. In this case, stoichiometry will help us find out how much CO2 can be produced from the given amounts of CaCO3 and HCl.
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Stoichiometry Concept
Limiting Reactant
The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. To identify the limiting reactant, we compare the mole ratios of the reactants used in the reaction to the stoichiometric coefficients in the balanced equation. The reactant that produces the lesser amount of product is the limiting reactant.
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01:30Limiting Reagent Concept
Gas Volume and Molar Volume
At standard temperature and pressure (STP), one mole of an ideal gas occupies 22.4 liters. This concept is crucial for converting moles of gas produced in a reaction to volume. In this problem, knowing that 1.00 mol of CO2 corresponds to 22.4 L allows us to calculate the volume of gas produced from the moles of CO2 generated by the reaction of the limiting reactant.
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Related Practice
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
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
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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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)2Cl2How 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
How many grams of the dry-cleaning solvent 1,2-dichloroethane (also called ethylene chloride), C2H4Cl2, can be prepared by reaction of 15.4 g of ethylene, C2H4, with 3.74 g of Cl2?
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