   Chapter 13, Problem 44E

Chapter
Section
Textbook Problem

# The reaction 2 NO ( g ) + Br 2 ( g ) ⇌ 2 NOBr ( g ) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.

Interpretation Introduction

Interpretation: The equilibrium constant value for the stated reaction is given 109 . The equilibrium partial pressure value of H2O and H2 is given. The partial pressure of NO at equilibrium 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 Kp .

To determine: The partial pressure of NO at equilibrium.

Explanation

Given

The stated reaction is,

2NO(g)+Br2(g)2NOBr(g)

The value of equilibrium constant Kp is 109 .

The equilibrium partial pressure of Br2 is 0.0159atm .

The equilibrium partial pressure of NOBr is 0.0768atm .

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

Kp=PartialpressureofproductsPartialpressureofreactants

Where,

• Kp is the equilibrium constant in terms of partial pressure.

The equilibrium ratio for the given reaction is,

Kp=(PNOBr)2(PNO)2(PBr2)

Substitute the given values of the equilibrium constant and the equilibrium partial pressure values of Br2 and NOBr in the above expression.

Kp=(PNOBr)2(PNO)2(PBr2)109=(0.0768)2(PNO)2(0

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