A) \[rate=k[A][B]\]
B) \[rate=k{{[A]}^{2}}\]
C) \[rate=k{{[A]}^{2}}{{[B]}^{1}}\]
D) \[rate=k{{[A]}^{2}}{{[B]}^{2}}\]
Correct Answer: B
Solution :
Let the rate of reaction depends on\[x\]th power of [A]. Then, \[{{r}_{1}}=k{{[A]}^{x}}\] and \[{{r}_{2}}=k{{[2A]}^{x}}\] \[\therefore \] \[\frac{{{r}_{1}}}{{{r}_{2}}}=\frac{{{[A]}^{x}}}{{{[2A]}^{x}}}=\frac{1}{4}={{\left( \frac{1}{2} \right)}^{2}}\] \[(\because {{r}_{2}}=4{{r}_{1}})\] \[\therefore \] \[x=2\] As the reaction rate does not depend upon the concentration of B. Hence, the correct rate-law will be rate \[k={{[A]}^{2}}{{[B]}^{0}}\]\[or=k{{[A]}^{2}}\]
You need to login to perform this action.
You will be redirected in
3 sec
