Consider the reaction A + B- P. Since the rate law could depend on both A & B, we take the following approach: First, we run the reaction with initial concentrations [B] = 0.1 M and [A] = 3.5 µM. We graph (1/M) as a function of time in seconds, and find that the data form a straight line. The equation is y 8.81 x 10 x + 2.9 x 105. We run the reaction again, but this time with initial concentrations [A] = 0.1 M and [B] = 3.5 µM. We graph In[B] as a function of time, and find that the data form a straight line. 1. What is the order of the reaction in A? 2. What is the order of the reaction in B? 3. What is the value of the rate constant? For the rate constant, the units will be some combination of mol, L, s. order in A Select one order in B Select one k enter value only, not units

Consider the reaction A + B- P. Since the rate law could depend on both A & B, we take the following approach: First, we run the reaction with initial concentrations [B] = 0.1 M and [A] = 3.5 µM. We graph (1/M) as a function of time in seconds, and find that the data form a straight line. The equation is y 8.81 x 10 x + 2.9 x 105. We run the reaction again, but this time with initial concentrations [A] = 0.1 M and [B] = 3.5 µM. We graph In[B] as a function of time, and find that the data form a straight line. 1. What is the order of the reaction in A? 2. What is the order of the reaction in B? 3. What is the value of the rate constant? For the rate constant, the units will be some combination of mol, L, s. order in A Select one order in B Select one k enter value only, not units

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Consider the reaction A + B- P.
Since the rate law could depend on both A & B, we take the following approach:
First, we run the reaction with initial concentrations [B] = 0.1 M and [A] = 3.5 UM. We graph (1/M) as a function of time in seconds, and find that the data form a
straight line. The equation is y = 8.81 x 10 3x + 2.9 x 105.
We run the reaction again, but this time with initial concentrations [A] = 0.1 M and [B] = 3.5 µM. We graph In[B] as a function of time, and find that the data form a
straight line.
1. What is the order of the reaction in A?
2. What is the order of the reaction in B?
3. What is the value of the rate constant? For the rate constant, the units will be some combination of mol. L.s.
order in A
Select one
order in B
Select one
k
enter value only, not units

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