Consider the following reaction: C_4H_8 (g) rightarrow 2 C_2H_4 (g) The followin

Question

Consider the following reaction: C_4H_8 (g) rightarrow 2 C_2H_4 (g) The following data were collected for the concentration for C_4H_8 as a function of time. a. What is the average rate of the reaction for C_4H_8 over the whole 50 seconds? b. What is the rate of the reaction for C_4H_8 between 0 and 10 seconds? c. How does the rate of the change over time? (Please describe why it changes as part of your answer.) d. What is the rate of formation of C_2H_4 between 0 and 10 seconds? e. Without making a graph, is there any way to determine whether this reaction is zero order in A? Explain.

Explanation / Answer

a)

AVG rate fr C4H8 over t = 50

AVG Rate = (Cf-Ci)/(Tf-Ti) = (0.637 - 1)/(50-0) = -0.00726 M/s

b)

rate changes over time:

As the time passes, the RATE is decreasing, that is, each time, the concentration changes vs. time LESS

c)

between 0 and 10:

AVG RAte = (Cf-Ci)/(Tf-Ti) = 0.913-1)/(10-0) = -0.0087 M/s

e)

Yes, if we calculate the SAME rate for each species, it will be zero order, since

Rate = Constant

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