Rate law for a gaseous reactionA+B→C+D is given byRate =K[A]2[B]0The volumes of reaction vessel containing these gases is suddenly reduced to one fourth the initial volume. The rate of reaction relative to original rate would be

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answer is B.

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Detailed Solution

On reducing the volume to ¼th increases the concentration of each reacting species four times. As rate is proportional to square of concentration of A and is independent of concentration of B rate increases sixteen times.

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