1. Consider the following generic reaction.

aA+bBcC+dDaA+bBcC+dD

A plot of log(rate)log(rate) versus log[A]log[A] when [B][B] is constant yields the following linear equation for its trendline.

=1.66+2.49=1.66+2.49

What is the order of the reaction with respect to A?

2. A plot of log(rate)log(rate) versus log[B]log[B] when [A][A] is constant yields the following linear equation for its trendline.

=0.97+2.91=0.97+2.91

What is the order of the reaction with respect to B?

3. What is the overall order of the reaction?

4.

Identify the rate law for this reaction.

rate=[A][B]2rate=[A][B]2

rate=[A]2[B]rate=[A]2[B]

rate=[A]2[B]2rate=[A]2[B]2

rate=[A][B]