Multiple Choice
The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl2(aq) + C2O4^2-(aq) → 2 Cl^-(aq) + 2 CO2(g) + Hg2Cl2(s). What is the rate law for the reaction?
15. Chemical Kinetics
Rate Law
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Based on the experimental data provided, what is the rate law for the reaction 2 NO (g) + 2 H2 (g) → N2 (g) + 2 H2O (g)?
A
Rate = k[NO]^1[H2]^1
B
Rate = k[NO]^2[H2]^1
C
Rate = k[NO]^1[H2]^2
D
Rate = k[NO]^2[H2]^2
Verified step by step guidance1
Understand the concept of a rate law: A rate law expresses the rate of a chemical reaction in terms of the concentration of the reactants. It is determined experimentally and can be represented as Rate = k[A]^m[B]^n, where k is the rate constant, [A] and [B] are the concentrations of the reactants, and m and n are the reaction orders with respect to each reactant.
Examine the given rate law: The problem provides a rate law as Rate = k[NO]^1[H2]^1. This suggests that the reaction is first order with respect to both NO and H2, meaning the rate is directly proportional to the concentration of each reactant.
Consider the experimental data: To determine the correct rate law, you would typically analyze experimental data showing how the rate changes with varying concentrations of NO and H2. This involves comparing initial rates of reaction at different concentrations to deduce the reaction orders.
Identify the correct rate law: Based on the options provided, the correct rate law is Rate = k[NO]^2[H2]^1. This indicates that the reaction is second order with respect to NO and first order with respect to H2, meaning the rate is proportional to the square of the concentration of NO and directly proportional to the concentration of H2.
Verify the rate law: To confirm the correct rate law, you would check if the experimental data supports the reaction orders of 2 for NO and 1 for H2. This involves ensuring that doubling the concentration of NO results in a fourfold increase in the rate, while doubling the concentration of H2 results in a twofold increase in the rate.
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