How long will it take for the concentration of A to decrease from 1.25 M to 0.287 for the second order reaction A → Products? (k = 1.52 M⁻¹min⁻¹)

Answer 1

Rate law for a 2nd order reaction is

1/[A] = 1/[A]_o + kt

[A]_o = 1.25 M

[A] = 0.287 M

k = 1.52 M^-1min^-1

t = ?

1/0.287 = 1/1.25 + 1.52t

3.48 = 0.80 + 1.52t

1.52 t = 2.68

t = 1.76 min