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Which one of following changes would result in greatest increase in reaction rate in the following two-step mechanism?

Step (i):$NO_2(g)+NO_2(g)\rightarrow NO(g)+NO_3(g)$[slow].

Step(ii):$NO_3(g)+CO(g)\rightarrow CO_2(g)+NO_2(g)$[fast).

$\begin{array}{1 1}(a)\;increase \;[CO]\\(b)\;increase\; [NO_2]\\(c)\;decrease\;[NO]\\(d)\;decrease\;[NO_3]\end{array}$

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Since rate is primarily decided by slowest step so when we increase the concentration of reactant of slowest step the rate of reaction automatically increases.
Hence (b) is the correct answer.
answered Dec 18, 2013 by sreemathi.v

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