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A reaction occurs by a two-step mechanism, shown below. Step 1: AX2(g) → AX(g) + X(g)...

A reaction occurs by a two-step mechanism, shown below. Step 1: AX2(g) → AX(g) + X(g) Step 2: AX2(g) + X(g) → AX + X2(g) The intermediate in this reaction is ________, and the molecularity of the second step is ________. Enter your answers separated by a comma.

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Answer #1

An Intermediate in a chemical reactcion is the specie that it is produced in one step of the process and consumed in a subsequent step to ultimately generate the final reaction product.

If we sum the steps of th reactions we can easily find that X(g) is formed in first step and consumed in the second Step.

So X(g) is the intermediate.

The molecularity of a chemical reaction is the number of molecules or ions that participate in that step. Then we can have unimolecular, bimolecular, termolecular, etc.

In the second step of the given reaction we have two species reacting: AX2(g) and X(g), then the step is bimolecular.

If you have any doubts please leave a comment :).

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