A) increase by 4 times
B) decrease by 2 times
C) increase by 2 times
D) remains the same
Correct Answer: C
Solution :
For the reaction: \[2A+B\xrightarrow{{}}{{A}_{2}}B\] \[r=k{{[A]}^{2}}[B]\] If concentration of A is doubled and that of B is halved, then \[r'={{[2A]}^{2}}\left[ \frac{B}{2} \right]\] \[2k{{[A]}^{2}}[B]\] \[r'=2r\] Hence, if the concentration of [A] is doubled and [B] is halved, then rate of reaction increases by 2 times.
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