Consider the hypothetical reaction A(g) + 2B(g) †’ C(g). The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0 L. The reaction is second order with respect to A and first order with respect to B.

a. Based on the information presented in the problem, write the rate law for the reaction.
b. Which of the containers, W, X, Y, or Z, would have the greatest reaction rate? Justify your answer.
c. Which of the containers would have the lowest reaction rate? Explain
d. If the volume of the container X were increased to 2.0 L, how would the rate of the reaction in this larger container compare to the rate of reaction run in the 1.0-L container X? (Assume that the number of A and B atoms is the same in each case.)
e. If the temperature in container W were increased, what impact would this probably have on the rate of reaction? Why?
f. If you want to double the rate of reaction in container X, what are some things that you could do to the concentration( s) of A and B?
g. In which container would you observe the slowest rate of formation of C?
h. Assuming that A and B are not in great excess, which would have the greater impact on the rate of reaction in container W: removing a unit of B or removing a unit of A? Explain.
i. Describe how the rate of consumption of A compares to the rate of consumption of B. If you cannot answer this question, what additional information do you need to provide an answer?
j. If the product C were removed from the container as it formed, what effect would this have on the rate of the reaction?

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