The following reaction occurs in basic solution: 

 OBr^—(aq) + PH₃(aq) → OH^—(aq) + PH₂Br(aq)

Given the initial rate data for the reaction at 25 °C, 

Determine the rate law for the reaction and numerical value of the rate constant, k, with correct units.

Given in the following table were the experimental data for the reaction 2 HCl(g) → H₂(g) + Cl₂(g). What concentration of HCl at 550 K would give a rate of 1.0×10⁻⁶ M/s?

The graph below shows the reaction rate vs the reactant concentration. Based on this graph, draw a plot of the concentration versus time. 

Identify the molecularity of each elementary reaction shown below.

The reaction 3 A + B → 2 C + D was proposed to observe the following three-step mechanism:

Step 1: A + B ⇌ F (fast)
Step 2: F + A → C + G (slow)
Step 3: G + A → C + D (fast)

What is the rate law predicted by the mechanism?

For the given elementary reaction equation

CO₂ (g) + NO (g) → CO (g) + NO₂(g)

a. Determine the order with respect to CO₂

b. Determine the overall order of the reaction

c. Identify the type of the elementary reaction (unimolecular, bimolecular, or termolecular)

PCl₅ decomposes to PCl₃ and Cl₂ in a gas-phase reaction at 200 °C: PCl₅(g) → PCl₃(g) + Cl₂(g)
The following data were obtained for the reaction:

Calculate the rate of the reaction at the following concentrations: 0.150 M, 0.200 M, and 0.230 M.

Consider the theoretical element A. "A" atoms combine to form A₂ is an aqueous solution. The reaction is second order and has a rate constant of 2.3 x 10¹⁰ M^-1s^-1. Assuming an initial concentration of 0.200 M, calculate the time it takes for 80% of the A atoms to convert to A₂.

The following data were gathered for the reaction

CD → C + D

Time(s)   [CD] (M)

0             1.00

10            0.833

20           0.714

30           0.625

40           0.555

50           0.505

60           0.455

Determine the following:

a. Order of the reaction

b. Rate constant of the reaction

c. Concentration of CD at 80 s

Two reactions were observed. The first reaction has a half-life that is twice as long as the last one. The second reaction has a half-life that is not affected by the concentration of the reactant and is constant over time. Identify the order of the rate law for each reaction based on the observations.

Consider the hypothetical decomposition reaction: AB → A + B. The following data were collected at 423.15 K:

t (s)           [AB] (M)
0.0           2.500
20.0         2.099
40.0         1.762
60.0         1.479
80.0         1.241
100.0        1.042

Calculate the half-life of the reaction at the initial concentration.