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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

Ammonia can decompose into its constituent elements according to the reaction

2 NH 3 ( g ) N 2 ( g ) + 3 H 2 ( g ) The equilibrium constant for the decomposition at a certain temperature is 2.5. Calculate the partial pressures of all the gases at equilibrium if ammonia with a pressure of 1.00 atm is sealed in a 3.0-L flask.

Interpretation Introduction

Interpretation:

The partial pressure of all the gases at equilibrium needs to be determined.

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 partial pressure of all the gases that is NH3(g), N2(g) and H2(g) needs to be calculated at equilibrium.

The given reaction is as follows:

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

The equilibrium constant for the reaction is 2.5.

The pressure of ammonia gas is 1.00 atm and volume is 3.0 L.

The partial pressure of all the gases can be calculated using the equilibrium reaction as follows:

2NH3(g)N2(g)+3H2(g)1                      -             -1-2p                p               3p

The expression for the equilibrium constant will be:

K=PN2

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