The rate equation of reaction is 2H2O2 → 2 H2O + O2 and the rate law for elementary step 1 is rate=k[H2O2][I−] .
The question is incomplete, the complete question is;
Step 1: H2O2 + I− → IO− + H2O
Step 2: H2O2 + IO− →H2O + O2 + I−
The mechanism for a chemical reaction is shown above. Which of the following statements about the overall reaction and rate laws of the elementary reactions is correct?
A) The chemical equation for the overall reaction is 2 H2O2+I−→ 2 H2O+O2+I− , and the rate law for elementary step 2 is rate=k[H2O2][IO−] .
B) The chemical equation for the overall reaction is H2O2+IO−→ H2O+O2+I− , and the rate law for elementary step 2 is rate=k[H2O2]2[IO−] .
C) The chemical equation for the overall reaction is 2 H2O2→2 H2O+O2 , and the rate law for elementary step 1 is rate=k[H2O2][I−] .
D) The chemical equation for the overall reaction is 2 H2O2→2 H2O+O2 , and the rate law for elementary step 1 is rate=k[H2O2]2 .
It is possible that a chemical reaction may not take place in a single reactive encounter. In that case, we can deduce the sequence of steps by which the reaction occurs. Each step is called an elementary reaction.
The overall rate law is the sum of all the elementary reactions after the intermediates have been eliminated. In this case, the specie IO− is an intermediate. Also, I− appears on both sides of the reaction equation and it has to cancel out.
The rate equation of reaction is 2H2O2 → 2H2O + O2 and the rate law for elementary step 1 is rate=k[H2O2][I−] .
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