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Chemistry: Principles and Reactions

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

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BuyFindarrow_forward

Chemistry: Principles and Reactions

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

Consider the hypothetical reaction at 325°C

R ( g ) + Q ( g ) 2 Z ( g ) K = 2.71

What are the equilibrium partial pressures of all the gases if all the gases (products and reactants) have an initial partial pressure of 0.228 atm?

Interpretation Introduction

Interpretation:

The partial pressure of Q, R and Z at equilibrium needs to be calculated.

Concept introduction:

For a general equilibrium 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.

Explanation

The given reaction is as follows:

R(g)+Q(g)2Z(g)

The equilibrium constant for the reaction is 2.71.

The initial partial pressure of all the gases is 0.228 atm.

The partial pressure at equilibrium can be calculated as follows:

R(g)+Q(g)2Z(g)0.228     0.228      0.2280.228-p   0.228-p  0.228+2p

The expression for the equilibrium constant will be as follows:

K=(PZ)2(PR)2(PQ)2

Putting the values,

2.71=(0.228+2p)(0.228+2p)(0.228p)(0

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