Question #32f3d
1 Answer
Answer:
Explanation:
We're asked to find the equilibrium pressures of the three gaseous substances in a reaction at a certain temperature, given the
Let's first write the equilibrium constant expression for this reaction:
We can set up I.C.E. chart (in the form of neat bullet points), starting with the initial quantities:
Initial:

#"COCl"_2# :#0.124# #"atm"# 
#"CO"# :#0# 
#"Cl"_2# :#0#
because only
According to the coefficients of the chemical equation, each species is in a
Change:
#"COCl"_2# :#x# 
#"CO"# :#+x# 
#"Cl"_2# :#+x#
Which means the final equilibrium pressures are

#"COCl"_2# :#0.124x# #"atm"# 
#"CO"# :#x# #"atm"# 
#"Cl"_2# :#x# #"atm"#
And we can plug these into our equilibriumconstant expression:
Solving for
The obvious value to use is the one that is both positive and not extreme (
The equilibrium partial pressures of each species is thus

#"COCl"_2# :#0.124(0.123996) = color(red)(4xx10^6# #color(red)("atm"# 
#"CO"# :#color(blue)(0.124# #color(blue)("atm"# 
#"Cl"_2# :#color(green)(0.124# #color(green)("atm"#
Our results reflect the pressure equilibrium lying far to the right.