Question

The rate constant for this zero‑order reaction is 0.0230 M ⋅ s − 1 at 300 ∘ C. A ⟶ products How long (in seconds) would it take for the concentration of A to decrease from 0.780 M to 0.220 M?

Answer 1

Answer:

$t=24.35\ seconds$

Explanation:

Using integrated rate law for first order kinetics as:

$[A_t] = [A_0]-kt$

Where,  

$[A_t]$ is the concentration at time t

$[A_0]$ is the initial concentration

Given that:

The rate constant, k = $0.0230$ Ms⁻¹

Initial concentration $[A_0]$ = 0.780 M

Final concentration $[A_t]$ = 0.220 M

Time = ?

Applying in the above equation, we get that:-

$0.220 = 0.780-0.0230\times t$

$780-23t=220$

$t=\frac{560}{23}$

$t=24.35\ seconds$