The following reaction is first order in A and first order in B:
A + B → Products Rate = k[A][B]
What is the initial rate of this reaction in vessel (b)relative to the initial rate of this reaction in vessel (a)? Each vessel has the same volume.Shaded spheres represent A molecules,and unshaded spheres represent B molecules present at the beginning of the reaction.

Question

Quizplus · Accepted Answer

The rate of the reaction is determined by the concentration of both A and B. In vessel (a), there are 2 A molecules and 2 B molecules, resulting in a rate of k[2][2] = 4k. In vessel (b), there are 2 A molecules and 1 B molecule, resulting in a rate of k[2][1] = 2k. Therefore, the ratio of the rate in vessel (b) to the rate in vessel (a) is 2:4 or simplified, 1:2. Thus, the correct answer is C.

The Following Reaction Is First Order in a and First