   Chapter 13, Problem 61E

Chapter
Section
Textbook Problem

# At 25°C, Kp = 2.9 × 10–3 for the reaction   NH 4 OCONH 2 ( s )   ⇌   2 NH 3 ( g )   +   CO 2 ( g )   In an experiment carried out at 25°C, a certain amount of NH4OCONH2 is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium.

Interpretation Introduction

Interpretation:

The equilibrium constant for the decomposition reaction of NH4OCONH2(s) is given. The value of total equilibrium pressure 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 equilibrium constant is 2.9×103 .

The stated reaction is,

NH4OCONH2(s)2NH3(g)+CO2(g)

It is assumed that the initial pressure of reactant is x and change in pressure of CO2 is y .

The initial pressure of product is,

(PNH3)= 0(PCO2)= 0

On the reaction with one molecule of NH4OCONH2(s) , the equilibrium reaction is,

NH4OCONH2(s)2NH3(g)CO2(g)Initialpressure:x0atm0atmChange(pressure):-y2yyEquilibrium(pressure):x-y2yy

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

Kp=ConcentrationofproductsConcentrationofreactants

Where,

• Kp is the equilibrium constant

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