The reaction A+B C + D has an initial rate of 0.0440 M/s. What will the initial rate be if [A] is halved and [B] is tripled? initial rate: rate = k[A][B]² What will the initial rate be if [A] is tripled and [B] is halved? initial rate: M/s M/s
The reaction A+B C + D has an initial rate of 0.0440 M/s. What will the initial rate be if [A] is halved and [B] is tripled? initial rate: rate = k[A][B]² What will the initial rate be if [A] is tripled and [B] is halved? initial rate: M/s M/s
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 2RQ: Distinguish between the differential rate law and the integrated rate law. Which of these is often...
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