15. Chemical Kinetics

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?

Which of the following is the correct expression for the rate of disappearance of NO(g) in the reaction 2 NO(g) + O_2(g) → 2 NO_2(g)?

Which of the following expressions correctly represents the rate constant, k, for a first-order reaction with respect to its half-life, t_{1/2}?

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

What is the rate law for the following elementary reaction: O3(g) + Cl(g) → O2(g) + ClO(g)?

For the zero-order reaction a → products, what is the rate when [a] = 0.200 M and k = 3.57 M/min?

What are the units of the rate constant k in the rate law: rate = k[x][y]?

What are the units of the rate constant k in the rate law: rate = k[x]^2[y]^2, where rate is in mol L^{-1} s^{-1} and concentrations are in mol L^{-1}?

Consider a multistep reaction where the slowest (rate-determining) step is: 2 NO_2(g) → NO_3(g) + NO(g). What is the best rate law for the overall reaction?

What are the units for the rate constant (k) of a first-order reaction?

Which of the following is a possible rate law for the reaction: a + b → c, if the reaction is first order in a and second order in b?

Which of the following expressions represents the rate at which ClO3^- (aq) is appearing in the reaction below?2 ClO2 (aq) + 2 OH^- (aq) → ClO3^- (aq) + ClO2^- (aq) + H2O (l)

What is the overall reaction order for the following rate law: rate = k[a][b][c]?