Question

consider the reaction below.
pcl₅(g) ←→ pcl₃(g) + cl₂(g)
at 500 k, the reaction is at equilibrium with the following concentrations.
pcl₅ = 0.0095 m
pcl₃ = 0.020
cl₂ = 0.020 m
what is the equilibrium constant for the given reaction?

Explanation:

Step1: Escribir la expresión de la constante de equilibrio

Para la reacción \( \text{PCl}_5(g)
ightleftharpoons \text{PCl}_3(g)+\text{Cl}_2(g) \), la constante de equilibrio \( K_c \) se define como \( K_c=\frac{[\text{PCl}_3][\text{Cl}_2]}{[\text{PCl}_5]} \)

Step2: Sustituir los valores de concentración

Dados \( [\text{PCl}_5]=0.0095\space M \), \( [\text{PCl}_3]=0.020\space M \) y \( [\text{Cl}_2]=0.020\space M \), sustituimos en la fórmula:
\( K_c=\frac{0.020\times0.020}{0.0095} \)

Step3: Realizar el cálculo

\( 0.020\times0.020 = 0.0004 \)
\( K_c=\frac{0.0004}{0.0095}\approx0.042 \)

Answer:

0.042