15. Chemical Kinetics

What is the rate expression for the disappearance of sulfur dioxide (SO2) in the reaction 2SO2(g) + O2(g) → 2SO3(g)?

Given the rate law: rate = k[a]^2[b], what is the order of the reaction with respect to a?

For the second-order reaction a → products, what is the rate when [a] = 0.201 M and k = 0.761 M^{-1} s^{-1}?

Using the information in the table below, determine the rate law for the reaction: a(g) + 3 b(g) → c(g) + 2 d(g). | Experiment | [a] (M) | [b] (M) | Initial Rate (M/s) | |------------|--------|--------|--------------------| | 1 | 0.10 | 0.10 | 0.020 | | 2 | 0.20 | 0.10 | 0.040 | | 3 | 0.10 | 0.20 | 0.080 | Which of the following is the correct rate law?

Which order of reaction produces a linear plot when concentration is graphed versus time?

For the reaction 2NO + O2 → 2NO2, the experimentally determined rate law is rate = k[NO]^2[O2]. What is the overall reaction order, what is the order with respect to O2, and what are the units of the rate constant k?

Which method can be used to determine the exponents in a rate law for a chemical reaction?

For the reaction with the rate law: rate = k[a]^2[b], what is the reaction order with respect to a?

Given the following reaction mechanism: Step 1: NO_2 + F_2 → NO_2F + F (slow) Step 2: F + NO_2 → NO_2F (fast) Which elementary step in the proposed mechanism is the rate-limiting step?

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?

Given that a plot of ln[reactant] versus time yields a straight line for a particular reaction, what is the order of this reaction?

Given the rate law for a reaction is rate = k[NO][O_2]^2 and the initial rate is 0.020 mol L^{-1} s^{-1} when [NO] = 0.10 mol L^{-1} and [O_2] = 0.20 mol L^{-1}, what is the value of the rate constant k at this temperature?

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?