Multiple Choice
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)?
15. Chemical Kinetics
Rate Law
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What is the rate law for the given mechanism in terms of the overall rate constant k, where Step 1 is fast and Step 2 is slow?
A
Rate = k[A][B]
B
Rate = k[A][B][C]
C
Rate = k[C]
D
Rate = k[D]
Verified step by step guidance1
Identify the slow step in the mechanism, as it determines the rate law for the overall reaction. In this case, Step 2 is the slow step.
Write the rate law expression for the slow step. Since Step 2 is slow, the rate law is determined by the reactants involved in this step.
Examine the given rate laws: Rate = k[A][B], Rate = k[A][B][C], Rate = k[C], Rate = k[D]. The correct rate law should reflect the reactants involved in the slow step.
Consider the role of intermediates and fast steps. If Step 1 is fast, it may establish an equilibrium that affects the concentration of reactants in the slow step.
Determine the overall rate law by considering the reactants involved in the slow step and any intermediates formed in the fast step. The correct rate law is Rate = k[C], indicating that C is the key reactant in the slow step.
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