The following reaction was monitored as a function of time: AB times A + B A plo
ID: 480488 • Letter: T
Question
The following reaction was monitored as a function of time: AB times A + B A plot of 1/[AB] versus time yields a straight line with slope 5.3 times 10^-2 (M middot s) You may want to reference section 15.5 while completing this problem. What is the half-life when the initial concentration is 0.55 M ? Express your answer using two significant figures. If the initial concentration of AB is 0.230 M, and the reaction mixture initially contains no products, what are the concentrations of A and B after 80 s ? Express your answers numerically using two significant figures, separated by a comma.Explanation / Answer
from the data it is clear that reaction is second order
for second order reaction.
t1/2 = 1/K[A0]
t1/2 = 1 / 0.053 [0.55]
t1/2 = 1 / 0.02915
t1/2 = 34 seconds
D) for second order
1/[A] = Kt + 1/[A0]
1/[A] = 0.053 x 80 + 1/0.23
1/[A] = 4.24 + 4.35
1/[A] = 8.59
[A] = 0.12 M
final concentration of [AB] = 0.12 M
0.23 - 0.12 = 0.11 M AB consumed
so [A] , [B] = 0.11 , 0.11
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