If a reaction is first order in A and zero order in B, what is the effect on the rate when [A] doubles at constant temperature?

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Multiple Choice

If a reaction is first order in A and zero order in B, what is the effect on the rate when [A] doubles at constant temperature?

Explanation:
When a reaction is first order in A and zero order in B, the rate law is rate = k[A][B]^0 = k[A]. With temperature fixed, the constant k does not change, so the rate depends only on [A]. Since rate is directly proportional to [A], doubling [A] doubles the rate. For example, if the original rate is R = k[A], then increasing A to 2[A] gives R' = k(2[A]) = 2R. The zero order in B means B has no effect on the rate at all.

When a reaction is first order in A and zero order in B, the rate law is rate = k[A][B]^0 = k[A]. With temperature fixed, the constant k does not change, so the rate depends only on [A]. Since rate is directly proportional to [A], doubling [A] doubles the rate. For example, if the original rate is R = k[A], then increasing A to 2[A] gives R' = k(2[A]) = 2R. The zero order in B means B has no effect on the rate at all.

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