An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of
ID: 852561 • Letter: A
Question
An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of mixing). The system then re-equilibrates. The appropriate chemical equation is:
PCl3(g) + Cl2(g) ---> PCl5(g)
Calculate the new partial pressures after equilibrium is reestablished.
PCl3 =
PCl2=
PCl5=
Please show all work in order to get credit, thanks!!!!
Explanation / Answer
PCl3(g) + Cl2(g) ---> PCl5(g)
13.2 13.2 217.0
13.2 +x 13.2 +x 217.0-x
Given 13.2+x +13.2+ x + 217.-x = 263.0
X = 19.6
new partial pressures after equilibrium is reestablished.
PCl3 = 13.2+19.6 = 32.8 torr
Cl2= 19.6 torr
PCl5= 217.0-19.6 197.6 torr