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Chapter 15: Problem 5

Define homogeneous equilibrium and heterogeneous equilibrium. Give two examples of each.

Short Answer

Expert verified
A homogeneous equilibrium is a state of balance in a chemical reaction where all reacting species are present in the same phase, as seen in example reactions \(N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)\) and \(H_2O(l) \leftrightharpoons H^+(aq) + OH^鈭�(aq)\). Conversely, a heterogeneous equilibrium is achieved when the reacting species exist in more than one phase, like in the reactions \(C(s) + CO_2(g) \rightarrow 2CO(g)\) and \(CaCO_3(s) \leftrightharpoons CaO(s) + CO_2(g)\).

Step by step solution

01

Define homogeneous equilibrium

A homogeneous equilibrium refers to a state of balance in a reaction where all reacting species are present in the same phase. This means that all substances, be it gases, liquids, or solids, exist in the same physical state.
02

Provide examples for homogeneous equilibrium

Example 1: \(N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)\). All constituents are in the gaseous phase. Example 2: \(H_2O(l) \leftrightharpoons H^+(aq) + OH^鈭�(aq)\). All constituents are dissolved in solution, thus considered the same phase.
03

Define heterogeneous equilibrium

A heterogeneous equilibrium refers to a state of balance in a reaction where the reacting species are present in more than one phase. The reacting species could be a combination of gases, liquids, solids, or even a substance dissolved in a solution.
04

Provide examples for heterogeneous equilibrium

Example 1: \(C(s) + CO_2(g) \rightarrow 2CO(g)\). The reactants and products are in both solid and gaseous phases.Example 2: \(CaCO_3(s) \leftrightharpoons CaO(s) + CO_2(g)\). The reactants and products are in both solid and gaseous phases.

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Most popular questions from this chapter

Consider the equilibrium system \(3 \mathrm{~A} \rightleftharpoons \mathrm{B}\). Sketch the change in concentrations of \(\mathrm{A}\) and \(\mathrm{B}\) with time for these situations: (a) Initially only A is present; (b) initially only B is present; (c) initially both \(\mathrm{A}\) and \(\mathrm{B}\) are present (with \(\mathrm{A}\) in higher concentration). In each case, assume that the concentration of \(\mathrm{B}\) is higher than that of \(\mathrm{A}\) at equilibrium.

When dissolved in water, glucose (corn sugar) and fructose (fruit sugar) exist in equilibrium as follows: fructose \(\rightleftharpoons\) glucose A chemist prepared a \(0.244 M\) fructose solution at \(25^{\circ} \mathrm{C}\). At equilibrium, it was found that its concentration had decreased to \(0.113 M\). (a) Calculate the equilibrium constant for the reaction. (b) At equilibrium, what percentage of fructose was converted to glucose?

(a) Use the van't Hoff equation in Problem 15.97 to derive the following expression, which relates the equilibrium constants at two different temperatures $$ \ln \frac{K_{1}}{K_{2}}=\frac{\Delta H^{\circ}}{R}\left(\frac{1}{T_{2}}-\frac{1}{T_{1}}\right) $$ How does this equation support the prediction based on Le Ch芒telier's principle about the shift in equilibrium with temperature? (b) The vapor pressures of water are \(31.82 \mathrm{mmHg}\) at \(30^{\circ} \mathrm{C}\) and \(92.51 \mathrm{mmHg}\) at \(50^{\circ} \mathrm{C} .\) Calculate the molar heat of vaporization of water.

A quantity of 0.20 mole of carbon dioxide was heated at a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: $$ \mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g) $$ Under this condition, the average molar mass of the gases was found to be \(35 \mathrm{~g} / \mathrm{mol}\). (a) Calculate the mole fractions of \(\mathrm{CO}\) and \(\mathrm{CO}_{2}\). (b) What is the \(K_{P}\) for the equilibrium if the total pressure was 11 atm? (Hint: The average molar mass is the sum of the products of the mole fraction of each gas and its molar mass.)

The equilibrium constant \(K_{P}\) for the reaction $$ 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g) $$ is \(5.60 \times 10^{4}\) at \(350^{\circ} \mathrm{C} . \mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) are mixed initially at 0.350 atm and 0.762 atm, respectively, at \(350^{\circ} \mathrm{C}\). When the mixture equilibrates, is the total pressure less than or greater than the sum of the initial pressures, 1.112 atm?
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