We’re being asked to determine the rate constant (k) of a second-order reaction:
N2O4 → 2 NO2
The integrated rate law for a second-order reaction is as follows:
[A]t = concentration at time t
k = rate constant
t = time
[A]0 = initial concentration
Given that N2O4 is 2nd order for the reaction: N2O4 → 2 NO2 , what is the concentration of N2O4 at 5 min when the rate constant is 0.50 min-1 M-1 and the initial [N2O4] is 0.24 M
A. 0.15 M
B. 6.7 M
C. 0.056 M
D. 0.22 M
E. 0.19 M
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