Chapter 13, Problem 114CP

### Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

Chapter
Section

### Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

# The equilibrium constant Kp for the reaction CCl 4 ( g ) ⇌ C ( s ) + 2 Cl 2 ( g ) at 700°C is 0.76. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C.

Interpretation Introduction

Interpretation: The initial pressure of carbon tetra-chloride is to be determined for the given reaction.

Concept introduction: The equilibrium constant Kc describes the ratio of the reactant to the product on the equilibrium conditions in terms of molar concentration.

The equilibrium constant depends upon temperature.

At equilibrium sum of all the partial pressure is equal to the total pressure.

Law of mass action is applicable on the equilibrium reactions.

Law of mass action states that at a given temperature the equilibrium constant is equal to the partial pressure of the products to the reactants raised the power of stoichiometric coefficient.

To determine: The initial pressure of CCl4 that produce a total equilibrium pressure of 1.20atm at 700°C .

Explanation

Explanation

Given

The reactions are given as,

CCl4(g)C(s)+2Cl2(g)

At 700°C the equilibrium constant in terms of partial pressure for the given reaction =0.76atm

Total equilibrium pressure at 700°C is 1.20atm

The initial pressure is assumed to be zatm and the change in pressure is assumed to be xatm is the change during the attainment of equilibrium. The ICE table is formed as follows.

InitialChangeEquilibriumCCl4(g)C(s)+2Cl2z0x+2xzx2x

Carbon is in solid form therefore its pressure is taken as unity.

At equilibrium the partial pressure is equal to the sum of the individual pressure of the all gases. Therefore,

Ptotal=Ppartial

Where,

• Ptotal is the total pressure at equilibrium.
• Ppartial is the partial pressure of the gases.
• represents the sum of all partial pressures.

Substitute the values of the equilibrium partial pressure in the above equation.

Ptotal=Ppartial1.20=zx+2x1.20=z+xz=1.20x (1)

The equilibrium constant in terms of partial pressure for the given reaction is given by the formula

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