A chemist conducts an experiment to determine the rate of the following reaction

Question

A chemist conducts an experiment to determine the rate of the following reaction:

A2 (g) + B2 (g) 2AB (g)

If the initial concentration of AB was 0.324 M and the concentration of AB was 0.838 M after 0.748 s, what is the average rate of the reaction?

Express your answer in units of M/s

If the same chemist performed another experiment under different conditions and determined that the initial concentration of A2 was 0.761 M and after 5.89 s the concentration of A2 was 0.340 M, what is the average rate of AB formation?

Express your answer in units of M/s

Explanation / Answer

1)
average rate of reaction = (1/2)*d[AB]/dt
= (1/2)*(C2-C1)/(t2-t1)
= (1/2)*(0.838 M - 0.324 M)/(0.748 s)
= 0.344 M/s
Answer: 0.344 M/s

2)
rate of reaction = (1/2)*d[AB]/dt = -d[A2]/dt
d[AB]/dt = -2*d[A2]/dt
So,
average rate of formation of AB = -2*(0.340 - 0.761) M / 5.89 s
= 0.143 M/s
Answer: 0.143 M/s

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