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 a reaction depends on the concentration of reactants. In vessel (a), there are 4 A molecules and 4 B molecules, so the initial rate of the reaction is proportional to [A][B] = 4x4 = 16. In vessel (b), there are 2 A molecules and 8 B molecules, so the initial rate of the reaction is proportional to [A][B] = 2x8 = 16, which is the same as in vessel (a). Therefore, the rate in vessel (b) is twice the rate in vessel (a), giving a ratio of 2:1. Therefore, the correct choice is C.

The Following Reaction Is First Order in a and First