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Chemistry / Chemistry 11 / Chapter 14 / Problem 62P

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

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Answer: Consider the following equilibrium reaction in a

Chapter 14, Problem 62P

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QUESTION:

Consider the following equilibrium reaction in a closed container:

\(\mathrm{CaCO}_{3}(s)\ \leftrightharpoons\ \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)\)

What will happen if (a) the volume is increased; (b) some CaO is added to the mixture; (c) some \(\mathrm{CaCO}_{3}\) is removed; (d) some \(\mathrm{CO}_{2}\) is added to the mixture; (e) a few drops of a NaOH solution are added to the mixture; (f) a few drops of a HCl solution are added to the mixture (ignore the reaction between \(\mathrm{CO}_{2}\) and water); (g) temperature is increased?

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QUESTION:

Consider the following equilibrium reaction in a closed container:

\(\mathrm{CaCO}_{3}(s)\ \leftrightharpoons\ \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)\)

What will happen if (a) the volume is increased; (b) some CaO is added to the mixture; (c) some \(\mathrm{CaCO}_{3}\) is removed; (d) some \(\mathrm{CO}_{2}\) is added to the mixture; (e) a few drops of a NaOH solution are added to the mixture; (f) a few drops of a HCl solution are added to the mixture (ignore the reaction between \(\mathrm{CO}_{2}\) and water); (g) temperature is increased?

ANSWER:

Step 1 of 8

The changes made in a reversible reaction will alter the equilibrium position to subsidize the difference, and Le Chatelier's principle studied this relation.

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