Ch.14 - Chemical Kinetics

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.14 - Chemical Kinetics

Problema 29a

Capitolo 14, Problema 29a

The decomposition reaction of N₂O₅ in carbon tetrachloride is 2 N₂O₅ → 4 NO₂ + O₂. The rate law is first order in N₂O₅. At 64°C the rate constant is 4.82 × 10^-3 s^-1. (a) Write the rate law for the reaction.

Guida verificata passo dopo passo

Identify the order of the reaction with respect to N2O5, which is given as first order.

Recall that the general form of a rate law for a first-order reaction is: rate = k[A], where k is the rate constant and [A] is the concentration of the reactant.

Substitute the given reactant, N2O5, into the rate law expression. The rate law becomes: rate = k[N2O5].

Use the given rate constant value, k = 4.82 \(\times\) 10^{-3} \(\text{ s}\)^{-1}, to complete the rate law expression.

The final rate law for the decomposition of N2O5 is: rate = 4.82 \(\times\) 10^{-3} \(\text{ s}\)^{-1} [\(\text{N}\)_2\(\text{O}\)_5].

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Rate Law

The rate law of a chemical reaction expresses the relationship between the rate of the reaction and the concentration of its reactants. It is typically formulated as rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B. In this case, since the reaction is first order in N2O5, the rate law will reflect that dependency.

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01:52

Rate Law Fundamentals

Order of Reaction

The order of a reaction indicates how the rate is affected by the concentration of reactants. A first-order reaction means that the rate is directly proportional to the concentration of one reactant raised to the first power. In the given reaction, the first-order nature in N2O5 implies that doubling its concentration will double the reaction rate.

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Average Bond Order

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that is specific to a particular reaction at a given temperature. It reflects the speed of the reaction; higher values of k indicate faster reactions. In this scenario, the rate constant is given as 4.82 * 10^-3 s^-1 at 64°C, which is crucial for calculating the reaction rate.

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01:14

Equilibrium Constant K

Pratica correlata

Domanda del libro di testo

Consider the following reaction: 2 NO1g2 + 2 H21g2¡N21g2 + 2 H2O1g2 (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and 3H24 is increased to 0.030 M?

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Domanda del libro di testo

The decomposition reaction of N₂O₅ in carbon tetrachloride is 2 N₂O₅ → 4 NO₂ + O₂. The rate law is first order in N₂O₅. At 64°C the rate constant is 4.82 × 10^-3 s^-1. (c) What happens to the rate when the concentration of N₂O₅ is doubled to 0.0480 M? (d) What happens to the rate when the concentration of N₂O₅ is halved to 0.0120 M?

Domanda del libro di testo

Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (b) How does the rate change when [A] is doubled and the other reactant concentrations are held constant? (c) How does the rate change when [B] is tripled and the other reactant concentrations are held constant? (d) How does the rate change when [C] is tripled and the other reactant concentrations are held constant? (f) By what factor does the rate change when the concentrations of all three reactants are cut in half?

Domanda del libro di testo

Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (a) Write the rate law for the reaction.

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Domanda del libro di testo

Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (e) By what factor does the rate change when the concentrations of all three reactants are tripled?

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Domanda del libro di testo

Consider the following reaction:

2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g)

(b) If the rate constant for this reaction at 1000 K is 6.0 × 10⁴ M^-2 s^-1, what is the reaction rate when [NO] = 0.035 M and [H₂] = 0.015 M?

(c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H₂ is 0.010 M?

The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5 → 4 NO2 + O2. The rate law is first order in N2O5. At 64°C the rate constant is 4.82 × 10-3 s-1. (a) Write the rate law for the reaction.

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Concetti chiave

Rate Law

Order of Reaction

Rate Constant (k)

The decomposition reaction of N₂O₅ in carbon tetrachloride is 2 N₂O₅ → 4 NO₂ + O₂. The rate law is first order in N₂O₅. At 64°C the rate constant is 4.82 × 10^-3 s^-1. (a) Write the rate law for the reaction.