15. Chemical Kinetics

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]?

Which of the following expressions correctly shows how the rate of a reaction depends on the concentrations of its reactants?

Given the reaction 2 w + x → y + z, and the following mechanism:Step 1: w + x → y (slow)Step 2: w + y → z (fast)What is the rate law for this reaction?

The concentration of N₂O was monitored at a constant temperature as a function of time for the reaction below.

N₂O (g) → N₂ (g) + ½ O₂ (g)

Reaction Time and Concentration of Nitrous Oxide

Time (s)	Molar Concentration [N2O]
0	0.500 M
20	0.382 M
40	0.310 M
60	0.260 M
80	0.224 M

Determine the rate law for this reaction.

What are the units of the rate constant k in the following rate law? rate = k [X]^0 [Y]^0