The enthalpy change of formation of PCl$_3$(g) under these conditions is provided. $\Delta H_f$ PCl$_3$(g) $= -320\,\text{kJ mol}^{-1}$. Calculate the enthalpy change of formation of PCl$_5$(g) under these conditions. Include a sign with your answer.
State and explain how increasing temperature affects the rate of decomposition of PCl$_5$(g).
State and explain how increasing temperature affects the percentage of PCl$_5$(g) that decomposes.
Explain the meaning of the term dynamic equilibrium and the conditions needed for it to be established.
At $450\,\text{K}$ and $1.00 \times 10^5\,\text{Pa}$, when $2.00\,\text{mol}$ of $\text{PCl}_5(g)$ decompose, the equilibrium mixture contains $0.800\,\text{mol}$ of $\text{Cl}_2(g)$. Calculate the partial pressure of phosphorus(V) chloride, $p\text{PCl}_5$, in this equilibrium mixture.
Write the equilibrium constant expression, $K_p$, for the decomposition of $\text{PCl}_5(g)$.
The partial pressures of $\text{PCl}_3(g)$ and $\text{Cl}_2(g)$ in this equilibrium mixture are each $2.86 \times 10^4\,\text{Pa}$. Calculate the value of $K_p$ and state its units.