For a first-order reaction the rate constant k ... - SS2 Chemistry Chemical Kinetics Question

Given: [A]₀ = 0.8 M, k = 0.02 s^-1, t = 30 seconds.

For a first-order reaction, the integrated rate law is given by:

[A] = [A]₀ x e^(-kt)

where [A] is the concentration of the reactant at time t, [A]₀ is the initial concentration, k is the rate constant, and e is the base of the natural logarithm.

Now, let's calculate the concentration of the reactant after 30 seconds:

[A] = 0.8 M x e^{(-0.02 s-1 x 30 s)}

[A] = 0.8 M x e^(-0.6)

[A] ≈ 0.8 M x 0.5488

[A] ≈ 0.439 M

So, the concentration of the reactant after 30 seconds is approximately 0.439 M.