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Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373

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Chapter
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BuyFindarrow_forward

Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373
Textbook Problem

The reversible reaction between hydrogen chloride gas and one mole of oxygen gas produces steam and chlorine gas:

4 HCl ( g ) + O 2 ( g ) 2 Cl 2 ( g ) + 2 H 2 O ( g ) K = 0.79

Predict the direction in which the system will move to reach equilibrium if one starts with

(a) P H 2 O = P HCl = P O 2 = 0.20 atm (b) P HCl = 0.30 atm, P H 2 O = 0.35 atm, P Cl 2 = 0.2 atm, P o 2 = 0.15 atm

Interpretation Introduction

(a)

Interpretation:

The direction of equilibrium needs to be determined for the given partial pressures of H2O, HCl and O2 gas.

Concept introduction:

The system is said to be in equilibrium if the there is no change in the partial pressure or concentration of reactant and product takes place.

For a general reaction as follows:

A(g)+B(g)C(g)+D(g)

The expression for the equilibrium constant is represented as follows:

K=(PC)(PD)(PA)(PB)

Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required.

If the value of reaction quotient of a reaction is less than the equilibrium constant, the reaction moves to forward direction and if the reaction quotient is more than equilibrium constant, the reaction moves to backward direction.

Explanation

The given reaction with the equilibrium constant value is as follows:

4HCl(g)+O2(g)2Cl2(g)+2H2O(g)     K=0.79

For the given values of partial pressure the reaction quotient can be calculated as follows:

Q=(PCl2)

Interpretation Introduction

(b)

Interpretation:

The direction of equilibrium needs to be determined for the given partial pressures of H2O, HCl, O2 and Cl2 gas..

Concept introduction:

The system is said to be in equilibrium if the there is no change in the partial pressure or concentration of reactant and product takes place.

For a general reaction as follows:

A(g)+B(g)C(g)+D(g)

The expression for the equilibrium constant is represented as follows:

K=(PC)(PD)(PA)(PB)

Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required.

If the value of reaction quotient of a reaction is less than the equilibrium constant, the reaction moves to forward direction and if the reaction quotient is more than equilibrium constant, the reaction moves to backward direction.

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