Answer to Question #174656 in General Chemistry for Jeneva

Question

Reaction 1:

Step 1 (slow): H2(g) + ICl(g) -> Hl(g)+ HCI(g)

Step 2 (fast): Hl(g) + ICl(g) -> I2(g) HCl(g)

a. Write the overall reaction. What substance is the reaction intermediate?

b. What is the rate law for the mechanism?

c. What is the molecularity of the mechanism?

Answer 1

a) HI(g)+ICl(g) ....fast

HCl(g)+I2(g)

b)it is the rate law for the slowest overall reaction, which is the same as the rate law for the slowest step in the reaction mechanism, the rate-determining step, that must give the experimentally determined rate law for the overall reaction.

c)Referring to the number of individual molecules involved in an elementary step of a reaction mechanism.