He rate law for the reaction 3 a c is rate = 4.36 ✕ 10-2 l mol-1 hr-1[a]2 what is the half-life for the reaction if the initial concentration of a is 0.250 m?

d[C] dt =.0436[A ]2 d[C] dt =.0436[A ]2

d[A] dt = - 3 d[C] dt d[A] dt = - 3 d[C] dt

d[A] dt = -.1308[A ]2 d[A] dt = -.1308[A ]2

- 1 [A ]2 d[A]=.1308dt - 1 [A ]2 d[A]=.1308dt

1 [A] =.1308t+C 1 [A] =.1308t+C

[A] = 1.1308t+C [A] = 1.1308t+C

.250 = 1C. 250 = 1C

C=4 C=4

.125 = 1.1308t+4.125 = 1.1308t+4

t = (1.125 - 4) ∗ 1.1308 = 30.58 t = (1.125 - 4) ∗ 1.1308 = 30.58

Assuming I did my math right, looks fine to me, it should be about 30 hours and 30 minutes.