What is the concentration of A after 13.3 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)

Question

this has to do with integrated rate law

Answer 1

First, based on the units of the rate constant (M^-1min^-1) we can tell this is a 2nd order reaction.

For a 2nd order reaction, we can use the following rate law:

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

[A] = concentration @ time t

[A]_o = initial concentration = 0.750 M

k = rate constant = 0.0451 M^-1min^-1

t = time = 13.3 min

1/[A] = 1/0.750 + (0.0451)(13.3)

1/[A] = 1.33 + 0.600

1/[A] = 1.93

[A] = 0.518 M