15. Chemical Kinetics

Considering the rate law, rate = k[a]^2[b], which of the following statements is correct?

Which of the following best describes the difference between the rate of a reaction and its rate constant?

Which of the following correctly matches the integrated rate law for a simple second-order reaction (where the rate depends on the concentration of a single reactant A)?

Given the rate law you determined for the reaction 2NO + O2 → 2NO2, which of the following expressions correctly represents the rate of the reaction if the rate law is rate = k[NO]^2[O2]?

Using the information in the table below, what is the correct rate law for the reaction 2 A(g) + B(g) → C(g) + D(g)?| Experiment | [A] (M) | [B] (M) | Initial Rate (M/s) ||------------|--------|--------|--------------------|| 1 | 0.10 | 0.10 | 2.0 × 10^{-3} || 2 | 0.20 | 0.10 | 4.0 × 10^{-3} || 3 | 0.10 | 0.20 | 2.0 × 10^{-3} |Which of the following is the correct rate law?

For the reaction: sucrose + H2O → glucose + fructose, the experimentally determined rate law is rate = k[sucrose][H2O]^0. What is the order of sucrose in the rate law for this reaction?

Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g). The experimentally determined rate law is: rate = k[NO]^2[O2]. Which of the following statements is correct regarding the reaction order?

What are the units for the rate constant (k) of a reaction with the rate law: rate = k[A][B]?

Which one of the following sets of units is appropriate for a second-order rate constant?

For a zeroth-order reaction, what are the units of the rate constant k?

Which of the following best describes what the rate law for a reaction shows?

Which of the following best describes a partial reaction order in a rate law?

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.