Calculate the equilibrium constant of the following reaction:
CO(g) + Cl₂(g) → COC12(g) AH = -112 kJ/mol
if the equilibrium concentrations of CO, Cl₂ and COCl₂ are 0.2 M, 0.1 M and 0.6 M respectively.
a) How will a decrease in temperature effect on equilibrium? Explain your answer.
b) How will an increase in pressure effect on equilibrium? Explain your answer
CO(g) + Cl₂(g) → COC12(g) AH = -112 kJ/mol
if the equilibrium concentrations of CO, Cl₂ and COCl₂ are 0.2 M, 0.1 M and 0.6 M respectively.
a) How will a decrease in temperature effect on equilibrium? Explain your answer.
b) How will an increase in pressure effect on equilibrium? Explain your answer
Answers & Comments
Answer:
COCl
2(g)
⇌CO
(g)
+Cl
2(g)
c−−⟹concentration
c−xxx⟹at equilibrium
K
c
=
[COCl
2
]
[CO][Cl
2
]
=
(c−x)
(x)(x)
Given, K
c
=0.08
c−x=0.1
K
c
=
c−x
x
2
⟹0.08=
0.1
x
2
x=0.0894≃0.09M
The equilibrium concentration of CO and Cl
2
are x=0.09m.
Answer:
COCl2 (g) at 740C are [CO] = 0.012 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M.
Explanation:
omogenous equilibrium applies to reactions in which all reacting species are in the same phase. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form