Problem 1 the experimentally determined rate law for the

Question

Problem 1: The experimentally determined rate law for the following reaction indicates that the reaction is second-order in AB and that the reaction is second-order overall.

AB + C → A + BC

a. Write the rate law for the reaction.

b. Is the following mechanism valid for this reaction? Provide TWO (2) reasons for your answer.

AB + AB → AB2 + A slow

AB₂ + C → AB + BC fast

c. When the temperature is increased from 25°C to 50°C, the reaction rate increases 1.65 times. What is the activation energy of the reaction?

d. Sketch the graph for the integrated rate law with respect to the concentration of AB.

Problem 2: For the reaction: 2A + B + 2C → D + E, the following initial rate data was collected at constant temperature.

Trial	[A]/M [B]/M		[C]/M	Rate/Ms-1
1	0.225	0.150	0.350	0.0217
2	0.320	0.150	0.350	0.0439
3	0.225	0.250	0.350	0.0362
4	0.225	0.150	0.600	0.01270

a. Determine the correct rate law for this reaction.

b. Calculate the rate constant, k.

c. Determine the reaction rate for A.

Problem 3: The data shown below were obtained from the following reaction: 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g)

Exp	[NO]0 (M)	[H2]0(M)	Initial Rate of Reaction (M/min)
1	0.0080	0.0060	4.3 10-4
2	0.0080	0.0120	8.6 10-4
3	0.0030	0.0080	8.0  10-5
4	0.0060	0.0080	3.2 10-4

a. Write the rate law for the reaction.

b. Calculate the value of the rate constant, k, for the reaction.

c. For experiment 2, calculate the concentration of NO remaining when exactly half of the original amount of H₂ has been consumed.

Problem 4: Iodine and propanone react in acid solution according to the following equation:

I₂(aq) = CH₃COCH₃(aq) →^H+ CH₃COCH₂I(aq) + HI(aq)

The experimentally determined rate law for this reaction indicates that the reaction is first-order in CH₃COCH₃ and first-order in H⁺. The reaction is second-order overall. At 50°C, the reaction rate is 2.00×10^-5 M/s when the concentration of CH₃COCH₃, I₂and H⁺ is1.50 M, 2.0x10^-2 M and 3.0x10^-2 M, respectively.

a. Calculate the rate constant at 50°C.

b. Calculate the rate of formation of CH₃COCH₂I when [I₂]= [ CH₃COCH₃]= [H⁺]= 2.00 M.

c. When the temperature is increased to 100°C, the reaction rate increases 1.5 times. What is the activation energy of the reaction?

d. What is the role of H⁺ in this reaction?

Problem 5: Gas phase dissociation reaction, A(g) ^→ B(g) + C(g) was monitored at 300^oC in terms of the decrease in the concentration of A with time as shown in TABLE

TABLE: Kinetics of Gas Phase Dissociation of A

Time (s)	[A] (M)
0	0.01000
100	0.00649
200	0.00481
300	0.00380

a. Determine the average rate of disappearance of A at 100 s.

b. Determine the reaction order by plotting the suitable graph(s) using data from TABLE

c. Write the rate law and determine the rate constant.

d. If at 400^oC the rate constant increased to 40.2 M^-1 s^-1, calculate the activation energy for the reaction.