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Consider the reaction below.



At 500 K, the reaction is at equilibrium with the following concentrations.

[PCI5]= 0.0095 M

[PCI3] = 0.020

[CI2] = 0.020 M


What is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24

Consider the reaction below At 500 K the reaction is at equilibrium with the following concentrations PCI5 00095 M PCI3 0020 CI2 0020 M What is the equilibrium class=

Respuesta :

Edufirst

Answer:

  • First choice: 0.042

Explanation:

Given decomposition reaction:

  • 1PCl₅ (g) ⇄ 1PCl₃ + 1Cl₂(g)

Equilibrium constant:

  • [tex]K_{eq}=\frac{[PCl_3]^1[Cl_2]^1}{[PCl_5]^1}[/tex]

Stoichiometric coefficients and powers equal to 1 are not usually shown as they are understood, but I included them in order to shwow you how they intervene in the equilibrium expressions: each concentration is raised to a power equal to the respective stoichiometric coefficient in the equilibrium equation.

So, your calculations are:

[tex]K_{eq}=\frac{(0.020M)(0.020M)}{0.0095M}=0.042M[/tex]

ItzDaGoofyGoober

Answer:

A

Explanation:

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