It is determined experimentally that the reaction E + F X + Y is second order wi

Question

It is determined experimentally that the reaction E + F X + Y is second order with respect to E and first order with respect to F. Which of the following statements is correct?

It is determined experimentally that the reaction E + F X + Y is second order with respect to E and first order with respect to F. Which of the following statements is correct?

Doubling the concentration of E will have no effect on the rate. Doubling the concentration of F will cause the reaction rate to increase by a factor of four. Halving the concentration of E will decrease the reaction rate by half. Doubling the concentration of E will increase the reaction rate by a factor of four.

Explanation / Answer

Option 1 is incorrect as rate=K[E]2[F]2 as rate will be four times

Option 2 is incorrect as rate becomes double

Option 3 is incorrect, rate becomes 1/4

Option 4 is correct, rate four times

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