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Chapter 14: Problem 83

Eggshells are composed mostly of calcium carbonate \(\left(\mathrm{CaCO}_{3}\right)\) formed by the reaction $$\mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q) \rightleftharpoons \mathrm{CaCO}_{3}(s)$$ The carbonate ions are supplied by carbon dioxide produced as a result of metabolism. Explain why eggshells are thinner in the summer when the rate of panting by chickens is greater. Suggest a remedy for this situation.

Short Answer

Expert verified
Eggshells are thinner in the summer because the rate of panting by chickens is greater. Panting removes more carbon dioxide, reducing the quantity of carbonate ions available for eggshell formation. This imbalance is counteracted by shifting the equilibrium of the reaction towards the formation of more calcium carbonate, thinning the eggshells. To remedy this situation, the amount of carbonate ions available for the reaction could be increased by introducing more calcium carbonate-rich meals into the chicken's diet.

Step by step solution

01

Understanding the Reaction

Eggshells are formed by a reversible reaction between calcium ions (\(\mathrm{Ca}^{2+}\)) and carbonate ions (\(\mathrm{CO}_{3}^{2-}\)) to form calcium carbonate (\(\mathrm{CaCO}_{3}\)). The carbonate ions are provided by carbon dioxide, a product of metabolism. In summer, chickens pant more to cool their bodies, which results in increased removal of carbon dioxide.
02

Explaining the Thinning of Eggshells

According to Le Chatelier's principle, if the concentration of any of the reactants or products in a reaction at equilibrium changes, the system will try to counteract that change. In this case, when chickens pant more, they exhale more carbon dioxide. This decrease in carbon dioxide reduces the number of carbonate ions available for the reaction. As a result, the system counteracts the change by moving the equilibrium to the right, encouraging the conversion of more \(\mathrm{Ca}^{2+}\) and \(\mathrm{CO}_{3}^{2-}\) to \(\mathrm{CaCO}_{3}\) to replenish the carbonate ions. Over time, this results in thinner eggshells.
03

Providing a Remedy

To remedy the situation, the amount of carbonate ions in the chicken's diet could be increased by adding more calcium carbonate-rich meals to their diet. This would provide more resources for eggshell formation, potentially counteracting the effects of the increased rate of panting and preserving the thickness of the eggshells.

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Most popular questions from this chapter

The equilibrium constant \(K_{\mathrm{c}}\) for the reaction \(2 \mathrm{NH}_{3}(g) \rightleftharpoons \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g)\) is 0.83 at \(375^{\circ} \mathrm{C} . \mathrm{A}\) 14.6-g sample of ammonia is placed in a \(4.00-\mathrm{L}\) flask and heated to \(375^{\circ} \mathrm{C}\). Calculate the concentrations of all the gases when equilibrium is reached.

Explain the difference between physical equilibrium and chemical equilibrium. Give two examples of each.

Define reaction quotient. How does it differ from equilibrium constant?

Write the equation relating \(K_{\mathrm{c}}\) to \(K_{P}\), and define all the terms.

At \(1024^{\circ} \mathrm{C},\) the pressure of oxygen gas from the decomposition of copper(II) oxide \((\mathrm{CuO})\) is 0.49 atm: $$4 \mathrm{CuO}(s) \rightleftharpoons 2 \mathrm{Cu}_{2} \mathrm{O}(s)+\mathrm{O}_{2}(g)$$ (a) What is \(K_{P}\) for the reaction? (b) Calculate the fraction of \(\mathrm{CuO}\) that will decompose if 0.16 mole of it is placed in a \(2.0-\mathrm{L}\) flask at \(1024^{\circ} \mathrm{C}\). (c) What would the fraction be if a 1.0 mole sample of \(\mathrm{CuO}\) were used? (d) What is the smallest amount of \(\mathrm{CuO}\) (in moles) that would establish the equilibrium?
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