Question

HCl can be produced by the exothermic reaction H2(g)+2ICl(g)→2HCl(g)+I2(g) . A proposed mechanism for the reaction has two elementary steps as shown below.

Step 1: H2(g)+ICl(g)→HI(g)+HCl(g) (slow)

Step 2: HI(g)+ICl(g)→HCl(g)+I2(g) (fast)
(d) Write a rate law for the overall reaction that is consistent with the proposed mechanism.
(e) On the incomplete reaction energy diagram below, draw a curve that shows the following two details.

The relative activation energies of the two elementary steps
The enthalpy change of the overall reaction

Answer 1

Answer:

Explanation:

The solutions and the answers can be found in the attachment

Answer 2

The rate of reaction can be given by Rate =  k $\rm H_2] [HCl]$.

The activation energy of step 1 is higher as compared to the activation energy of step 2.

• In the proposed mechanism for the formation of HCl, two steps have been followed.

The rate of reaction has been determined by the slow step.

Thus the rate will be:

Rate = k $\rm H_2] [HCl]$,

where k is the rate constant.

• In the incomplete diagram, the wave for step 1 has higher activation energy as it has been a slow step.

The activation energy of step 2 has been lower as compared to step 1.

For more information about the rate of reaction, refer to the link:

https://brainly.com/question/25159894