We’re being asked to calculate the half-life of a second-order reaction with a rate constant of 0.50 min-1 M-1 initially at 0.75 M
Recall that half-life (t1/2) is the time needed for the amount of a reactant to decrease by 50% or one-half. The half-life of a second-order reaction is given by:
k = rate constant
[A]0 = initial concentration
Given that N2O4 is 2nd order for the reaction: N2O4 → 2 NO2, if a reaction started with 0.75 M N2O4, what is the half-time when the rate constant is 0.50 min-1 M-1
A. 1.33 min
B. 2.25 min
C. 0.50 min
D. 2.67 min
E. 10.3 min
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