Question

1) Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures:

CO(g)+Cl2(g)?COCl2(g)

Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 459?C . At equilibrium, the concentrations were measured and the following results obtained:

Gas	Partial Pressure (atm)
CO	0.880
Cl2	1.18
COCl2	0.200

What is the equilibrium constant, Kp, of this reaction?

2) In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.

Part B

The following reaction was performed in a sealed vessel at 753?C :

H2(g)+I2(g)?2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.35M and [I2]=2.15M. The equilibrium concentration of I2 is 0.0500M . What is the equilibrium constant, Kc, for the reaction at this temperature?

Express your answer numerically.

Answer 1

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Part A

Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures:

CO(g)+Cl2(g)?COCl2(g)

Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 476?C . At equilibrium, the concentrations were measured and the following results obtained:

Gas	Partial Pressure (atm)
CO	0.840
Cl2	1.16
COCl2	0.140

What is the equilibrium constant, Kp, of this reaction?

In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.

Part B

The following reaction was performed in a sealed vessel at 725?C :

H2(g)+I2(g)?2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=4.00M and[I2]=2.55M. The equilibrium concentration of I2 is 0.0100M . What is the equilibrium constant, Kc, for the reaction at this temperature?

Step1 Kp =Pcocl2/PcoxPcl2 = .140/.840x1.16 =.144

QB Step1 I2 used in reaction = 2.55-.01=2.54M ; H2 used in reaction = 2.54M ;

Step2 At equalibrium [H2] = 4.00-2.54=1.46M ; [I2]=.01M ; [HI] =5.08M

Step3 Kc = 5.08x5.08/1.46x.01 = 1768