Given the following equation for the reaction between A and B: 2A + 3B → C
If the reaction is first order with respect to A and second order with respect to B. The rate law is

Question

Given the following equation for the reaction between A and B: 2A +  3B →  C
If the reaction is first order with respect to A and second order with respect to B. The rate law is

BlackTom AI · Accepted Answer

The problem states that the reaction is first order with respect to A and second order with respect to B, so the rate law must reflect those orders in the exponents of the concentrations of A and B.

Option a: Rate = k[A][B]. This would imply first order in A and first order in B. Since the problem specifies second order in B, this option is inconsistent with the given information and thus incorrect.

Option b: Rate = k[A][B]2. This expression correctly assigns a first-order dependence on A (exponent 1) and a second-order dependence on B (exponent 2), matching the stated reaction orders. Therefore, this option aligns with the described kinetics.

Option c: Rate = k[A]2[B]3. Here, the order with respect to A is 2 and with respect to B is 3. Both of these exponents contradict the given first-order in A and second-order in B, making this option incorrect.

Option d: Rate = k[A]2[B]. This scenario gives a second order in A and first order in B, again conflicting with the stated orders and thus not permissible based on the information provided.

In summary, only the expression in option b satisfies the specified reaction orders (first order in A, second order in B), while the others misrepresent the kinetic orders required by the problem.

Given the following equation for the reaction between A and B: 2A + 3B → C If the reaction is first order with respect to A and second order with respect to B. The rate law isSingle choice

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