The proposed 3-step mechanism for a reaction is Step 1) X(g) + Y(g) A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k-1 = reverse rate constant.) Step 2) A(g) + Z(g) B(g) slow (k2 = rate constant) Step 3) B(g) P(g) fast (k3 = rate constant) a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your
The proposed 3-step mechanism for a reaction is
Step 1) X(g) + Y(g) A(g) fast, reaches equilibrium
(For Step 1, k1 = forward rate constant & k-1 = reverse rate constant.)
Step 2) A(g) + Z(g) B(g) slow (k2 = rate constant)
Step 3) B(g) P(g) fast (k3 = rate constant)
a) What is the overall reaction?
b) What is the rate law supported by this mechanism? Explain your answer.
c) The following is experimental data found for this reaction:
| Initial [X] (M) | Initial [Y] (M) | Initial [Z] (M) | Initial Rate (M/day) | |
| Exp 1 | 0.150 | 0.150 | 0.150 | 0.569 |
| Exp 2 | 0.250 | 0.150 | 0.150 | 0.948 |
| Exp 3 | 0.250 | 0.300 | 0.150 | 3.793 |
| Exp 4 | 0.300 | 0.350 | 0.200 | 6.196 |
i) What is the experimentally determined rate law?
ii) Determine the rate constant and include units.
d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer.
e) ΔΔHo = -347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism. Label your profile with the proper reactants, products, and intermediates. Indicate where the activated complexes would be. You can write the activated complexes as 'AC'. Be sure to label your axis.
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