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11 Nov 2019
Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reacion rte constant 1 | rate constant NO2(g)--NO(g) + O(g) Suppose also k,ok. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical rate Note: your answer should not contain the concentrations of any intermediates Express the rate constant k for the overall chemical reaction in terms of ki, k2, and (if necessary) the rate L constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.
Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reacion rte constant 1 | rate constant NO2(g)--NO(g) + O(g) Suppose also k,ok. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical rate Note: your answer should not contain the concentrations of any intermediates Express the rate constant k for the overall chemical reaction in terms of ki, k2, and (if necessary) the rate L constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.
Jean KeelingLv2
15 Jun 2019