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A reaction, A + B -> C, is considered second order with respect to A and first order with respect to B. What is the effect of simultaneously doubling the concentration of A and B on the rate of reaction?

"second order with respect to A" tells us that doubling the concentration of A will cause the reaction rate to increase by a factor of 4."first order with respect to B" then tells us that doubling the concentration of B will cause the reaction rate to double.If these changes of concentration occur simultaneously the the reaction rate increases by a factor of 8 ie. 2x4=8 for the combined effect of doubling both concentrations.

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A reaction, A + B -> C, is considered second order with respect to A and first order with respect to B. What is the effect of simultaneously doubling the concentration of A and B on the rate of reaction?

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