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Chapter 16: Problem 23

What is a homogeneous equilibrium system? Give an example of a homogeneous equilibrium reaction. What is a heterogeneous equilibrium system? Write two chemical equations that represent heterogeneous equilibria.

Short Answer

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A homogeneous equilibrium system is a chemical system where all reactants and products are in the same phase, such as the reaction between nitrogen gas and hydrogen gas to form ammonia gas: \(N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)\). A heterogeneous equilibrium system involves reactants and products in different phases, like the reaction between calcium carbonate (solid) and heat: \(CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)\), or the reaction between water (liquid) and carbon dioxide (gaseous) to form carbonic acid (aqueous): \(CO_2(g) + H_2O(l) \rightleftharpoons H_2CO_3(aq)\).

Step by step solution

01

Homogeneous Equilibrium System

A homogeneous equilibrium system is a chemical system in which all the reactants and products are present in the same phase (solid, liquid or gas). That is, all components exist in a single, homogenous mixture.
02

Example of a Homogeneous Equilibrium Reaction

An example of a homogeneous equilibrium reaction is the reaction between nitrogen gas and hydrogen gas to form ammonia gas: \[N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)\] In this reaction, all the reactants and products are in the gaseous phase.
03

Heterogeneous Equilibrium System

A heterogeneous equilibrium system is a chemical system in which the reactants and products are present in different phases (solid, liquid, or gas). In other words, the components in a heterogeneous equilibrium system coexist in separate, distinct phases.
04

Chemical Equations Representing Heterogeneous Equilibria (1)

One example of a heterogeneous equilibrium system is the reaction between calcium carbonate (solid) and heat, which results in calcium oxide (solid) and carbon dioxide (gaseous): \[CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)\] In this reaction, we have a solid reactant converting into a solid product and a gaseous product.
05

Chemical Equations Representing Heterogeneous Equilibria (2)

Another example of a heterogeneous equilibrium system is the reaction between water (liquid) and carbon dioxide (gaseous), which forms carbonic acid (aqueous): \[CO_2(g) + H_2O(l) \rightleftharpoons H_2CO_3(aq)\] Here, we have a gaseous reactant and a liquid reactant combining to form an aqueous product. This is also a heterogeneous equilibrium system, as the reactants and product exist in different phases.

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Most popular questions from this chapter

Write the equilibrium expression for each of the following reactions. a. \(4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightleftharpoons 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\) b. \(2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)\) c. \(\mathrm{CH}_{3} \mathrm{OH}(g) \rightleftharpoons \mathrm{CH}_{2} \mathrm{O}(g)+\mathrm{H}_{2}(g)\)

As you know from Chapter \(7,\) most metal carbonate salts are sparingly soluble in water. Below are listed several metal carbonates along with their solubility products, \(K_{\mathrm{sp}} .\) For each salt, write the equation showing the ionization of the salt in water, and calculate the solubility of the salt in mol/L. $$\begin{aligned}&\text { Salt } \quad K_{\mathrm{sp}}\\\&\mathrm{BaCO}_{3} \quad 5.1 \times 10^{-9}\\\&\mathrm{CdCO}_{3} \quad 5.2 \times 10^{-12}\\\&\mathrm{CaCO}_{3} \quad 2.8 \times 10^{-9}\\\&\mathrm{CoCO}_{3} \quad 1.5 \times 10^{-13}\end{aligned}$$

In your own words, describe what Le Ch谩telier's principle tells us about how we can change the position of a reaction system at equilibrium.

The solubility product of iron(III) hydroxide is very small: \(K_{\mathrm{sp}}=4 \times 10^{-38}\) at \(25^{\circ} \mathrm{C} .\) A classical method of analysis for unknown samples containing iron is to add \(\mathrm{NaOH}\) or \(\mathrm{NH}_{3}\). This precipitates \(\mathrm{Fe}(\mathrm{OH})_{3}\) which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of \(\mathrm{Fe}(\mathrm{OH})_{3}\) in moles per liter and in grams per liter.

Zinc carbonate, \(\mathrm{ZnCO}_{3}(\mathrm{s}),\) dissolves in water to give a solution that is \(1.7 \times 10^{-5} \mathrm{M}\) at \(22^{\circ} \mathrm{C}\). Calculate \(K_{\mathrm{sp}}\) for \(\mathrm{ZnCO}_{3}(s)\) at this temperature..
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