A certain gas mixture is held at #395^@ "C"# has the following initial partial pressures: #P_(Cl_2) = 351.4#, #P_(CO) = 342.0#, #P_(COCl_2) = 0#, all in #"torr"#. Find #K_P^@#?
At equilibrium, the total pressure is #"439.5 torr"# . #V# is held constant. Find #K_P^@ = (P_(COCl_2)/P^@)/((P_(Cl_2)/P^@)(P_(CO)/P^@))# for
#"CO"(g) + "Cl"_2(g) rightleftharpoons "COCl"_2(g)#
at #395^@ "C"# , where #P^@ = "750.062 torr"# (and #chi_AP_"tot" = n_A/(n_"tot")P_"tot" = P_A# , the partial pressure of #A# ).
My guess is somehow I have to find the partial pressures at equilibrium, but there's not enough obvious information for me to immediately figure this out.
At equilibrium, the total pressure is
#"CO"(g) + "Cl"_2(g) rightleftharpoons "COCl"_2(g)#
at
My guess is somehow I have to find the partial pressures at equilibrium, but there's not enough obvious information for me to immediately figure this out.
1 Answer
Since Michael and Stefan managed to help me to figure this out, I'll put an answer here.
We got
The main idea is that for ideal gases, at fixed
#sum_i^N P_i = P_1 + P_2 + . . . + P_N = P_"tot"#
which we will use for
First, we can construct an ICE table to determine the expression for each equilibrium partial pressure.
#"CO"(g) " "+" " "Cl"_2(g) " "rightleftharpoons" " "COCl"_2(g)#
#"I"" "342.0" "" "" "351.4" "" "" "" "" "0#
#"C"" "-x" "" "" "-x" "" "" "" "" "+x#
#"E"" "342.0-x" "351.4-x" "" "" "x#
The equilibrium partial pressures can be expressed as Dalton's Law of partial pressures:
#P_"CO" + P_("Cl"_2) + P_("COCl"_2) = P_("tot",eq) = "439.5 torr"#
#342.0 - x + 351.4 cancel(- x + x) = 439.5#
#693.4 - x = 439.5#
#color(green)(x) = 693.4 - 439.5 = color(green)("253.9 torr")#
From this, we can construct the expression to calculate
#color(blue)(K_P^@) = (P_(COCl_2)/P^@)/((P_(Cl_2)/P^@)(P_(CO)/P^@))#
#= ((253.9)/(750.062))/(((351.4 - 253.9)/(750.062))((342.0 - 253.9)/(750.062))#
#= color(blue)(22.17)#
