A sealed flask with a volume of $1\,\text{dm}^3$ is used to heat one mole of phosphorus(V) chloride, $\text{PCl}_5$, to $600\,\text{K}$. Once equilibrium has been reached, measurements are recorded. $\text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g)$ The experiment is then carried out again, but this time one mole of phosphorus(V) chloride is heated to $600\,\text{K}$ in a sealed flask of volume $2\,\text{dm}^3$. How will the measurements vary?
- AThe equilibrium concentrations of $\text{PCl}_3(g)$ and $\text{Cl}_2(g)$ are higher in the second experiment.
- BThe equilibrium concentration of $\text{PCl}_5(g)$ is lower in the second experiment.
- CThe equilibrium concentrations of all three gases are the same in both experiments.
- DThe value of the equilibrium constant is higher in the second experiment.