The following reaction is second order in A and first order in B:
A + B → Products Rate = k[A]²[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

The following reaction is second order in A and first order in B: A + B → Products Rate = k[A]<sup>2</sup>[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. A) rate in vessel (b) /rate in vessel (a) = 1:2 B) rate in vessel (b) /rate in vessel (a) = 1:1 C) rate in vessel (b) /rate in vessel (a) = 2:1 D) rate in vessel (b) /rate in vessel (a) = 4:1

Quizplus · Accepted Answer

The Answer of The following reaction is second order in A and first order in B: A + B → Products Rate = k[A]²[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.

The Following Reaction Is Second Order in a and First