Textbook Question
A reaction A + B → C obeys the following rate law: Rate = k[B]2. (a) If [A] is doubled, how will the rate change? Will the rate constant change?
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Ch.14 - Chemical Kinetics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 14, Problem 25b
(b) The reaction 2 NO1g2 + Cl21g2¡2 NOCl1g2 is carried out in a closed vessel. If the partial pressure of NO is decreasing at the rate of 56 torr/min, what is the rate of change of the total pressure of the vessel?
Verified step by step guidance1
Identify the stoichiometry of the reaction: For every 2 moles of NO and 1 mole of Cl2, 2 moles of NOCl are produced. The reaction can be written as: 2 NO(g) + Cl2(g) → 2 NOCl(g).
Determine the rate of consumption of Cl2 based on the stoichiometry. Since 2 moles of NO react with 1 mole of Cl2, the rate of decrease in Cl2's partial pressure will be half the rate of decrease of NO's partial pressure.
Calculate the rate of formation of NOCl. According to the stoichiometry, 2 moles of NOCl are formed for every 2 moles of NO consumed. Thus, the rate of increase in NOCl's partial pressure will be equal to the rate of decrease of NO's partial pressure.
Sum up the rates of change in partial pressures. The total pressure change in the vessel is the sum of the rate of decrease of NO and Cl2 partial pressures and the rate of increase of NOCl partial pressure.
Apply the ideal gas law if necessary, considering the volume and temperature are constant in a closed vessel, to relate the changes in partial pressures directly to changes in the number of moles of gases.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Partial Pressure
Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. Understanding how partial pressures relate to the total pressure is crucial for analyzing gas reactions and their rates.
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Rate of Reaction
The rate of reaction refers to the change in concentration of reactants or products over time. In this context, the rate at which the partial pressure of NO is decreasing indicates how quickly the reaction is proceeding. This rate can be used to determine the changes in total pressure based on stoichiometric relationships in the balanced chemical equation.
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Stoichiometry
Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In the given reaction, the stoichiometric coefficients indicate that for every 2 moles of NO consumed, 2 moles of NOCl are produced. This relationship is essential for calculating how changes in the concentration or pressure of one component affect the total pressure in the system.
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Related Practice
Textbook Question
For each of the following gas-phase reactions, indicate how the rate of disappearance of each reactant is related to the rate of appearance of each product:
(d) C2H5NH2(g) → C2H4(g) + NH3(g)
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Textbook Question
For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant:
(a) 2 H2O(g) → 2 H2(g) + O2(g)
(b) 2 SO2(g) + O2(g) → 2 SO3(g)
(c) 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)
(d) N2(g) + 2 H2(g) → N2H4(g)
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Textbook Question
For each of the following gas-phase reactions, indicate how the rate of disappearance of each reactant is related to the rate of appearance of each product:
(a) H2O2(g) → H2(g) + O2(g)
(b) 2 N2O(g) → 2 N2(g) + O2(g)
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Textbook Question
A reaction A + B → C obeys the following rate law: Rate = k[B]2. (b) What are the reaction orders for A and B? What is the overall reaction order?
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