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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 :

dsdrajlin

Answer:

0.406 M

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.

[tex][Cl_2O_5] = [Cl_2O_5]_0 \times e^{-k \times t}[/tex]

where,

  • [Cl₂O₅]₀: initial concentration
  • t: time elapsed

[tex][Cl_2O_5] = 1.16 M \times e^{-0.184 s^{-1} \times 5.70s} = 0.406 M[/tex]

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