   Chapter 13, Problem 30E

Chapter
Section
Textbook Problem

# The following equilibrium pressures were observed at a certain temperature for the reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 NH 3 ( g )           P NH 3 = 3.1 × 10 − 2 atm               P N 2 = 8.5 × 10 − 1 atm               P H 2 = 3.1 × 10 − 3 atm Calculate the value for the equilibrium constant Kp at this temperature.If P N 2 = 0.525   atm P NH 3 = 0.0167 atm, and P H 2 = 0.00761 atm. does this represent a system at equilibrium?

Interpretation Introduction

Interpretation: The partial pressure values of N2 , H2 and NH3 at a particular temperature are given. The value of the equilibrium constant (Kp) for the given reaction is to be calculated. A comment on the equilibrium state for the reaction with the reactants having the given partial pressure values is to be determined.

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 equilibrium constant (Kp) for the given reaction.

Explanation

Given

The stated reaction is,

N2(g)+3H2(g)2NH3(g)

The partial pressure value for NH3 (PNH3) is 3.1×102atm .

The partial pressure value for N2 (PN2) is 8.5×101atm .

The partial pressure value for H2 (PH2) is 3.1×103atm .

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=(PNH3)2(PN2)(PH2)3

Substitute the given partial pressure values in the above expression.

Kp=(3.1×102)2(8.5×101)(3.1×103)3=3

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