Phosphorus pentachloride decomposes according to the chemical equation

$PC{l}_5(g)PC{l}_3(g)+C{l}_2(g),K_c=1\mathrm{.}80at250C$

A $0\mathrm{.}2293$mol sample of $PC{l}_5(g)$ is injected into an empty $3\mathrm{.}15L$ reaction vessel held at $250C.$

Calculate the concentrations of $PC{l}_5(g)$ and $PC{l}_3(g)$ at equilibrium.

$[PC{l}_5]=$

M

$[PC{l}_3]=$