Question

1.Part A The activation energy of a certain reaction is 43.7 kJ/mol . At 29 ∘C , the rate constant is 0.0150s−1 . At what temperature in degrees Celsius would this reaction go twice as fast? Part B Given that the initial rate constant is 0.0150s−1 at an initial temperature of 29 ∘C , what would the rate constant be at a temperature of 170. ∘C for the same reaction described in Part A?

2. Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 2X→Y+Z 2. Y+2L→M+Z Part 1: What is the rate law for step 1 of this reaction? Part 2: What is the rate law for step 2 of this reaction?

3. The relative rates of the reaction 2A+C2→2AC in vessels (1)-(4) are 1:1:2:3. Red spheres represent A molecules, blue spheres represent B molecules, and connected yellow spheres represent C2 molecules. Write a mechanism that agrees with the rate law?

Answer 1