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Phosphine (PH3) decomposes into phosphorus and molecular hydrogen:
4PH3(g) → P4(g) + 6H2(g)
Experiments show that this is a first-order reaction, with a rate constant of 0.0173 s-1 at 650°C. Identify each of the following statements about this reaction as true or false. (Use the drop-down menu and select "True" or "False" for each. You must get all 4 correct.)
TrueFalse The rate constant would be smaller than 0.0173 s-1 at 590°C.
TrueFalse The reaction PH3 → PH2 + H might be the rate-determining step in the mechanism of this reaction.
TrueFalse The mechanism for this reaction must involve two or more elementary steps.
TrueFalse The data given would allow us to determine the activation energy for the reaction.

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Patrina Schowalter
Patrina SchowalterLv2
29 Sep 2019

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Related questions

Phosphine (PH3) decomposes into phosphorus and molecular hydrogen:
4PH3(g) → P4(g) + 6H2(g)
Experiments show that this is a first-order reaction, with a rate constant of 0.0173 s-1 at 650°C. Identify each of the following statements about this reaction as true or false. (Use the drop-down menu and select "True" or "False" for each. You must get all 4 correct.)
True/False The mechanism for this reaction must involve two or more elementary steps.
True/False The activation energy for the reaction cannot be determined without additional data.
True/False The rate constant would be smaller than 0.0173 s-1 at 500°C.
True/False The rate-determining step for the reaction could involve a bimolecular collision between two PH3 molecules.

Consider the reaction below:

2NO2(g) + F2(g) ⟶ 2NO2F(g)

a. Based on the information provided in the table below (all measurements are at 25 ºC), determine the

experimental rate law and calculate the rate constant at this temperature. You can assume ideal gas

behavior for both NO2 and F2.

Initial Pressures (atm) Experiment p(NO2); p(F2) (mol L-1 s-1)

1) .038 ; .060

2) .076 ; .060

3) .076 ; .030

Initial Rate

1 0.038 0.060 1.4  10– 5

2 0.076 0.060 2.8  10– 5

3 0.076 0.030 1.4  10– 5

b. Contrasting NO2 and F2, which one of these two real gases would be closer to ideal gas assumed in part a?

Draw the Lewis structures of both to support your argument.

c. Based on the rate law determined in part a, propose a reaction mechanism comprising of two bimolecular

elementary steps. Hint: F is an intermediate in the overall reaction.

d. Which elementary process in part c is rate-determining?

e. You conduct experiment 1 from the table in part a. If your initial p(NO2) is 0.038 atm and p(F2) is kept at

constant flow of 0.060 atm, how long would it take for the pressure of NO2 to drop to 0.001 atm?

f. The collision frequency and steric factor for the rate-determining step in the overall process at 25 ºC are

5.9x1010 and 0.16, respectively. Calculate the activation energy (in kJ/mol) for the rate determining step.

g. If the enthalpy of reaction (i.e. standard enthalpy change for the overall process) is -100 kJ/mol, sketch the

energy profile of the two-step reaction given that i) the activation energy for the fast step in part c is 5

kJ/mol and ii) equilibrium partial pressures of all species involved in the fast step are 1.0 atm

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