A) \[Rate=k[A]\,[B]\]
B) \[Rate=\frac{k}{4}{{[A]}^{2}}\]
C) \[Rate=k{{[A]}^{2}}[B]\]
D) \[Rate=k{{[A]}^{2}}{{[B]}^{2}}\]
Correct Answer: B
Solution :
\[2A+B\xrightarrow{{}}Product\] ...(i) Doubling the concentration of A cause the reaction. rate to be four time so order of reaction is two. \[A+2B\xrightarrow{{}}Product\] ... (ii) Doubling the concentration of B does not effect the rate so, order of reaction is zero. So equation no. (i) \[4\times Rate\,\alpha {{[A]}^{2}}\]\[4\times Rate\,=k{{[A]}^{2}}\]or \[Rate\,=\frac{k{{[A]}^{2}}}{4}\] where, k = velocity constant
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