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For the reaction at 500 K NO_(2)(g)+CO(g) to CO_(2)(g)+NO(g) The proposed mechanism is as follows: (i) NO_(2)+NO_(2) to NO+NO_(3) (slow) (ii) NO_(3)+CO to CO_(2)+NO_(2) (fast) What is the rate law for the reaction? |
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Answer» Solution :Rate LAW : `(dx)/(dt)=K[NO_(2)]^(2)` Thus is because the SLOW step determines the rate of reaction and there are two `NO_(2)` reactant molecules in the slow step of the reaction. |
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