Textbook Question
This reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. a. Calculate the rate of the reaction when [N2O5] = 0.055 M
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Ch.14 - Chemical Kinetics
Chapter 14, Problem 39b
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C. b. What is the overall order of the reaction?
Verified step by step guidance1
Identify the order of the reaction with respect to each reactant: first order in A, second order in B, and zero order in C.
Recall that the overall order of a reaction is the sum of the orders with respect to each reactant.
Add the orders of the reactants: first order (A) + second order (B) + zero order (C).
Calculate the sum: 1 (from A) + 2 (from B) + 0 (from C).
The overall order of the reaction is the result of this sum.
Verified Solution
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reaction Order
The reaction order is a key concept in chemical kinetics that indicates the relationship between the concentration of reactants and the rate of the reaction. It is determined by the sum of the powers of the concentration terms in the rate law. For example, if a reaction is first order in A and second order in B, the overall order is the sum of these orders.
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Average Bond Order
Rate Law
The rate law expresses the rate of a chemical reaction as a function of the concentration of its reactants, each raised to a power corresponding to its order in the reaction. The general form is Rate = k[A]^m[B]^n[C]^p, where k is the rate constant, and m, n, and p are the orders with respect to reactants A, B, and C, respectively. Understanding the rate law is essential for determining the overall order of the reaction.
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01:52Rate Law Fundamentals
Zero Order Reactions
In zero order reactions, the rate of reaction is independent of the concentration of the reactant. This means that changes in the concentration of a zero-order reactant do not affect the rate of the reaction. In the given question, since C is zero order, it does not contribute to the overall order, which is calculated solely from the other reactants.
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Related Practice
Textbook Question
This reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. b. What would the rate of the reaction be at the concentration indicated in part a if the reaction were second order? Zero order? (Assume the same numerical value for the rate constant with the appropriate units.)
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Textbook Question
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.
a. Write a rate law for the reaction.
Textbook Question
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. a. Write a rate law for the reaction.
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Open Question
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. b. What is the overall order of the reaction? order in A, one-half order in B, and second order in C
Open Question
Consider the data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.