Domanda del libro di testo
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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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 14, Problema 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?
Guida verificata passo dopo passo1
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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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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Percorso guidato
00:48
Partial Pressure Calculation
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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Percorso guidato
02:03Average Rate of Reaction
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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Percorso guidato
01:16Stoichiometry Concept
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