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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 \(H_2O(l) \leftrightharpoons H^+(aq) + OH^−(aq)\). 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: \(H_2O(l) \leftrightharpoons H^+(aq) + OH^−(aq)\). 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

The vapor pressure of mercury is \(0.0020 \mathrm{mmHg}\) at \(26^{\circ} \mathrm{C}\). (a) Calculate \(K_{\mathrm{c}}\) and \(K_{P}\) for the process \(\mathrm{Hg}(l) \rightleftharpoons \mathrm{Hg}(g) .\) (b) A chemist breaks a thermometer and spills mercury onto the floor of a laboratory measuring \(6.1 \mathrm{~m}\) long, \(5.3 \mathrm{~m}\) wide, and \(3.1 \mathrm{~m}\) high. Calculate the mass of mercury (in grams) vaporized at equilibrium and the concentration of mercury vapor in \(\mathrm{mg} / \mathrm{m}^{3}\). Does this concentration exceed the safety limit of \(0.050 \mathrm{mg} / \mathrm{m}^{3} ?\) (Ignore the volume of furniture and other objects in the laboratory.)

Consider the equilibrium $$ 2 \mathrm{I}(g) \rightleftharpoons \mathrm{I}_{2}(g) $$ What would be the effect on the position of equilibrium of (a) increasing the total pressure on the system by decreasing its volume, (b) adding \(I_{2}\) to the reaction mixture, (c) decreasing the temperature?

In this chapter we learned that a catalyst has no effect on the position of an equilibrium because it speeds up both the forward and reverse rates to the same extent. To test this statement, consider a situation in which an equilibrium of the type $$ 2 \mathrm{~A}(g) \rightleftharpoons \mathrm{B}(g) $$ is established inside a cylinder fitted with a weightless piston. The piston is attached by a string to the cover of a box containing a catalyst. When the piston moves upward (expanding against atmospheric pressure), the cover is lifted and the catalyst is exposed to the gases. When the piston moves downward, the box is closed. Assume that the catalyst speeds up the forward reaction \((2 \mathrm{~A} \longrightarrow \mathrm{B})\) but does not affect the reverse process \((\mathrm{B} \longrightarrow 2 \mathrm{~A})\). Suppose the catalyst is suddenly exposed to the equilibrium system as shown below. Describe what would happen subsequently. How does this "thought" experiment convince you that no such catalyst can exist?

The dissociation of molecular iodine into iodine atoms is represented as $$ \mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g) $$ At \(1000 \mathrm{~K}\), the equilibrium constant \(K_{\mathrm{c}}\) for the reaction is \(3.80 \times 10^{-5}\). Suppose you start with 0.0456 mole of \(I_{2}\) in a 2.30 - \(L\) flask at \(1000 \mathrm{~K}\). What are the concentrations of the gases at equilibrium?

Write the equilibrium constant expressions for \(K_{\mathrm{c}}\) and \(K_{P}\), if applicable, for these reactions: (a) \(2 \mathrm{NO}_{2}(g)+7 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)\) (b) \(2 \mathrm{ZnS}(s)+3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{ZnO}(s)+2 \mathrm{SO}_{2}(g)\) (c) \(\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)\) (d) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}(a q) \rightleftharpoons \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-}(a q)+\mathrm{H}^{+}(a q)\)
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