Question

The rate constant for this zero‑order reaction is 0.0130 M ⋅ s − 1 0.0130 M·s−1 at 300 ∘ C. 300 ∘C. A ⟶ products A⟶products How long (in seconds) would it take for the concentration of A A to decrease from 0.890 M 0.890 M to 0.280 M? 0.280 M? t = t= s

Answer 1

The time is 46.9s

Step-by-step explanation:

The general formula for a zero-order reaction is:

[A] = -kt + [A]₀ (1)

Where: [A] is concentration in time t, k is rate constant and [A]₀ is initial concentration. Replacing the values of the problem in (1):

0.280M = -0.0130Ms⁻¹ₓ t + 0.890M

-0.610M = -0.0130Ms⁻¹ₓ t

-0.610M / -0.0130Ms⁻¹ = t

46.9s = t

The time is 46.9s

I hope it helps!