   Chapter 13, Problem 62E

Chapter
Section
Textbook Problem

# A sample of solid ammonium chloride was placed in an evacuated container and then heated so that it decomposed to ammonia gas and hydrogen chloride gas. After heating, the total pressure in the container was found to be 4.4 atm. Calculate Kp at this temperature for the decomposition reaction     NH 4 Cl ( s )   ⇌   NH 3 ( g )   +   HCl ( g )

Interpretation Introduction

Interpretation:

The total pressure for the decomposition reaction of ammonium chloride [NH4Cl(s)] is given.  The value of equilibrium constant is to be calculated.

Concept introduction:

The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.  When the equilibrium constant is expressed in terms of pressure, it is represented as Kp .

Explanation

Given

The total pressure of given reaction is 4.4atm .

The stated reaction is,

NH4Cl(s)NH3(g)+HCl(g)

The initial pressure of product is,

(PNH3)= 0(PHCl)= 0

It is assumed that the change in pressure of HCl is x .

The equilibrium expression is not applied for solids. On the reaction with one molecule of NH4Cl(s) , the equilibrium reaction is,

NH4Cl(s)NH3(g)HCl(g)Initialpressure:1.0atm0atm0atmChange(pressure):0xxEquilibrium(pressure):1.0atmxx

At equilibrium, the equilibrium ratio is expressed by the formula,

Kp=ConcentrationofproductsConcentrationofreactants

Where,

Kp is the equilibrium constant

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