For the reaction x_2+ y + z → xy + xz, it is found that the rate equation is rate = k [x_2][y]. which of the following might explain why the concentration of z has no effect on the rate?

a. the concentration of z is very small and the others are very large.
b. z must react in a step other than the rate determining step.
c. z is an intermediate.
d. the fraction of molecules of z that have very high energies is zero.
e. the activation energy for z to react is very low.

 C. Z is an intermediate.

Explanation:  The given reaction is

And the rate equation is rate =  k [X_2][Y]

From this, we can imply that either the concentration of Z is very small in comparison tot he other reactants or the reactant Z is an intermediate which is available only for the given small amount of time.

There can be various steps in the mechanism for the proposed reaction and Z can also react in any of the steps. It is not necessary that it should react in a step other than the rate determining step.

This might be possible that the activation energy for Z to react is very low But since it has made a new kind of product that is XZ, then the former cannot be true.

because of all the things that happen around the us, many people get into arguments which sadly could get physical, but we should actually make a change for that.