5. The following mechanism is proposed for the reaction between hydrogen and iodine monochloride: Step 1: H2 + ICl→HI + HCl Step 2: HI + ICl→I2 + HCl
a. Write the balanced equation for the overall reaction. All components are gaseous.
b. Identify any intermediate(s) and/or catalyst(s) in the reaction.
c. If the first step is slow, what would you expect to be the rate law for the overall reaction?
d. If the second step is slow, and the first step is fast and reversible, what do you expect to be the rate law for the overall reaction?
e. If the following data were obtained, which mechanism is supported? Explain.
Time (s) 0
50.0 100.0 200.0 300.0
[ICl] (M) .01000 .00787 .00649 .00481 .00380