Question

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.184 s^-1 ? Suppose a vessel contains Cl_2 O_5 at a concentration of 1.16 M. Calculate the concentration of Cl_2 O_5 in the vessel 5.70 seconds later. You may assume no other reaction is important.

Answer 1

0.406 M

Step-by-step explanation:

Let's consider the following reaction.

2 Cl₂O₅(g) → 2 Cl₂(g) + 5 O₂(g)

This reaction follows first-order kinetics with a rate constant (k) of 0.184 s⁻¹.

We can calculate the concentration [Cl₂O₅] at a certain time using the following expression.

`[Cl_2O_5] = [Cl_2O_5]_0 * e^(-k * t)`

where,

• [Cl₂O₅]₀: initial concentration

• t: time elapsed

`[Cl_2O_5] = 1.16 M * e^{-0.184 s^(-1) * 5.70s} = 0.406 M`