15. Chemical Kinetics

For a reaction that is second order overall, what are the units of the rate constant k?

Consider the following rate law: rate = k[a]^n[b]^m. How are the exponents n and m determined?

For the reaction a → b, if the reaction is first order with respect to a and the rate constant is k, which of the following is the correct rate law?

Given the reaction a → b, if the rate constant k is 0.25 mol L^{-1} s^{-1} at 75 °C and the reaction is first order in a, what is the correct rate law for this reaction?

Which of the following is the correct rate law for the elementary reaction: O3(g) + O(g) → 2O2(g)?

For the uncatalyzed reaction 2NO + O2 → 2NO2, which of the following is the correct rate law?

Which of the following would be a reasonable unit for the rate constant of a zero order reaction?

Given the reaction A + B → C + D and the following experimental data:| Experiment | [A] (M) | [B] (M) | Initial Rate (M/s) ||------------|---------|---------|--------------------|| 1 | 0.10 | 0.10 | 2.0 × 10^{-4} || 2 | 0.20 | 0.10 | 4.0 × 10^{-4} || 3 | 0.10 | 0.20 | 2.0 × 10^{-4} |Which of the following is the correct rate law for this reaction?

Which of the following is the correct rate law for the reaction between HCl and Na2S2O3, assuming the reaction is first order with respect to each reactant?

Consider the reaction mechanism:Step 1: NO_2 + F_2 → NO_2F + FStep 2: NO_2 + F → NO_2FIf the second step is rate determining, what is the correct rate law expression for the overall reaction?

Given the reaction mechanism:Step 1: NO_2 + F_2 → NO_2F + F (slow)Step 2: F + NO_2 → NO_2F (fast)What is the rate law for the overall reaction based on this mechanism?

Given the following data for the reaction A + B → products:| [A] (mol/L) | [B] (mol/L) | Initial Rate (mol/L·s) ||-------------|-------------|------------------------|| 0.10 | 0.10 | 0.020 || 0.20 | 0.10 | 0.040 || 0.10 | 0.20 | 0.040 |Assuming the rate law is rate = k[A][B], what is the value of the rate constant k (in L/mol·s)?

Given the reaction 2NO + O_2 → 2NO_2 and the following initial rate data:| [NO] (M) | [O_2] (M) | Initial Rate (M/s) ||----------|-----------|---------------------|| 0.10 | 0.10 | 1.2 × 10^{-3} || 0.20 | 0.10 | 4.8 × 10^{-3} || 0.10 | 0.20 | 2.4 × 10^{-3} |Determine the correct rate law and value of the rate constant k.

For a second-order reaction, what are the units for the rate constant k?

For the reaction x + 2 y → xy₂, if the reaction occurs in a single elementary step as proposed, what is the correct rate law?