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Question

The reaction 2A + B + C → D + E is found to be first-order in A, second order in B and zero-order in C. What is the effect on the rate of increasing concentration of A, B, and C two times?

A
72 times
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B
8 times
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C
32 times
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D
None of these
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Solution

The correct option is B 8 times
The reaction 2A + B + C → D + E is first-order in A, second in B and zero-order in C.
Thus the rate of the reaction, r = k [A]¹ [B]² [C]⁰. The overall rate of the reaction is of third order. Since the rate of reaction is independent of [C]; so A and B will only affect rate of reaction by a factor of (2 x 2²) = 8.
Hence, option B is correct.

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