consider the reaction below.\npcl₅(g)⇌pcl₃(g) + cl₂(g)\nat 500 k, the reaction is at equilibrium with the…

consider the reaction below.\npcl₅(g)⇌pcl₃(g) + cl₂(g)\nat 500 k, the reaction is at equilibrium with the following concentrations.\npcl₅= 0.0095 m\npcl₃ = 0.020\ncl₂ = 0.020 m\nwhat is the equilibrium constant for the given reaction?\n0.042\n0.42\n2.4\n24

consider the reaction below.\npcl₅(g)⇌pcl₃(g) + cl₂(g)\nat 500 k, the reaction is at equilibrium with the following concentrations.\npcl₅= 0.0095 m\npcl₃ = 0.020\ncl₂ = 0.020 m\nwhat is the equilibrium constant for the given reaction?\n0.042\n0.42\n2.4\n24

Answer

Explanation:

Step1: Write equilibrium - constant expression

For the reaction $\text{PCl}{5}(g)\rightleftharpoons\text{PCl}{3}(g)+\text{Cl}{2}(g)$, the equilibrium - constant expression $K_c$ is $K_c=\frac{[\text{PCl}{3}][\text{Cl}{2}]}{[\text{PCl}{5}]}$.

Step2: Substitute the given concentrations

Substitute $[\text{PCl}{5}]=0.0095\ M$, $[\text{PCl}{3}]=0.020\ M$, and $[\text{Cl}_{2}]=0.020\ M$ into the expression: $K_c=\frac{0.020\times0.020}{0.0095}$.

Step3: Calculate the value of $K_c$

$K_c=\frac{0.0004}{0.0095}\approx0.042$.

Answer:

0.042