Part A

Consider the second-order reaction:

2HI(g)→H2(g)+I2(g)

Rate law: k[H]^2

k= 6.4*10^-9 (mol*s) at 500 K

Initial rate = 1.6 * 10^-7 mol (l*s)

What will be the concentration of HI after t =3.65×10¹⁰ s ([HI]t) for a reaction startingunder this condition?

Part B

In a study of the decomposition of the compound X via thereaction

X(g)⇌Y(g)+Z(g)

the following concentration-time data were collected:

Time (min)	[X](M)
0	0.467
1	0.267
2	0.187
3	0.144
4	0.117
5	0.099
6	0.085
7	0.075

Given that the rate constant for the decomposition ofhypothetical compound X from part A is 1.60 M−1⋅min−1,calculate the concentration of X after 14.0 min .

Part C

The following data were collected for the rate of disappearanceof NO in the reaction2NO(g)+O2(g)→2NO2(g):

Experiment	[NO](M)	[O2](M)	Initial Rate (M/s)
1	0.0126	0.0125	1.41×10−2
2	0.0252	0.0250	1.13×10−1
3	0.0252	0.0125	5.64×10−2

What is the rate of disappearance of NO when [NO]=6.15×10^{−2} M and [O2]=1.75×10^{−2} M ?

Part D

What is the rate of disappearance of O2 at the concentrationsgiven in part (c)?

Part E

A certain reaction with an activation energy of 175 kJ/mol wasrun at 515 K and again at 535 K . What is the ratio of fat the higher temperature to f at the lowertemperature?

Usef=e^−Ea/(R⋅T)