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

`t=24.35\ seconds`

Step-by-step 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* t`

`780-23t=220`

`t=(560)/(23)`

`t=24.35\ seconds`