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Chemistry / Chemistry 11 / Chapter 14 / Problem 89P

Chemistry | 11th Edition | ISBN: 9780073402680 | Authors: Raymond Chang

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Chapter 14, Problem 89P

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QUESTION:

A mixture containing 3.9 moles of NO and 0.88 mole of \(\mathrm{CO}_{2}\) was allowed to react in a flask at a certain temperature according to the equation

\(\mathrm{NO}(g)+\mathrm{CO}_{2}(g)\ \leftrightharpoons\ \mathrm{NO}_{2}(g)+\mathrm{CO}(g)\)

At equilibrium, 0.11 mole of \(\mathrm{CO}_{2}\) was present. Calculate the equilibrium constant \(K_{c}\) of this reaction.

Questions & Answers

QUESTION:

A mixture containing 3.9 moles of NO and 0.88 mole of \(\mathrm{CO}_{2}\) was allowed to react in a flask at a certain temperature according to the equation

\(\mathrm{NO}(g)+\mathrm{CO}_{2}(g)\ \leftrightharpoons\ \mathrm{NO}_{2}(g)+\mathrm{CO}(g)\)

At equilibrium, 0.11 mole of \(\mathrm{CO}_{2}\) was present. Calculate the equilibrium constant \(K_{c}\) of this reaction.

ANSWER:

Step 1 of 6

Given:

The initial moles of

The initial moles of

The moles of carbon dioxide at equilibrium is .

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