| The reaction, \[X+2Y+Z\to N\] occurs by the following mechanism |
| (i) \[X+Y\rightleftharpoons M\] (very rapid equilibrium) |
| (ii) \[M+Z\to O\](slow) |
| (iii) \[O+Y~\to N\](very fast) |
| What is the rate law for this reaction? |
A) Rate = k[Z]
B) Rate = k[X] \[{{[Y]}^{2}}\] [Z]
C) Rate = k[N]
D) Rate = k[X] [Y] [Z]
Correct Answer: D
Solution :
[d] \[{{K}_{C}}=\frac{[M]}{[X][Y]}\Rightarrow [M]={{K}_{C}}[X][Y]\] Rate\[=K'[M][Z]=K'{{K}_{C}}[X][Y][Z]\] \[=K[X][Y][Z]\]
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