Terms relating to certain types of substances are conventionally omitted from equilibrium constant expressions. These substances are

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In discussing equilibrium constant expressions, certain substances are conventionally omitted from the expression.

First, consider what goes into an equilibrium constant expression: we use activities (effective concentrations or pressures) of the species involved.

Next, recall that for a pure solid or a pure liquid, its activity is essentially a constant and does not change with amount in the container. Therefore, multiplying by or dividing by that constant does not affect the value of the equilibrium constant.

Because activities of pure solids and pure liquids are taken as 1 in the context of the equilibrium expression, their concentrations are not included in the K expression. This makes the expression depend only on the activities of the species present in the more variable phases, typically gases and in solution.

If there were multiple-choice options, the correct choice would identify pure solids and liquids as the substances whose terms are omitted in the equilibrium constant expression.

Note: in this particular item, the answer choices are not provided, so the discussion focuses on the standard rationale behind omitting these phases rather than selecting among listed options.

Terms relating to certain types of substances are conventionally omitted from equilibrium constant expressions. These substances are

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Terms relating to certain types of substances are conventionally omitted from equilibrium constant expressions. These substances are

查看解析

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类似问题

Methanol is manufactured by the following exothermic reaction. CO (g) + 2H2 (g) ⇌ CH3OH (g) Which pair of changes will favour the forward reaction?[Fill in the blank]

Chemical equilibrium is the state where chemical reactions are in balance and no longer occurring.

For the reaction N2(g) + 3 H2(g) 2 NH3(g) Kc = 0.0600 at a certain temperature. In an equilibrium mixture of the three gases, [NH3] = 0.242 M and [ H2] = 1.03 M. What is the concentration of N2 in this system?

Which of the following statements concerning equilibrium constants is true?

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: What is the equilibrium concentration of ICl if 0.75 mol of I2 and 0.75 mol of Cl2 are initially mixed in a 2.0-L flask?

Consider the equilibrium system C(s) + CO2(g) ⇔2CO(g) If C is removed, the equilibrium will _____, and if CO is added, the equilibrium will _____.

Consider the equilibrium reaction: CO (g) + H2 (g) ⇌ C (s) + H2O (g), ΔHr = –131.3 kJ mol–1 Making use of Le Chatelier’s principle, identify which of the following will happen if the temperature of the system is increased.

2SO2 (g) + O2 (g) ⇌ 2SO3 (g) For this exothermic reaction, the equilibrium constant, K = 781. If, after equilibrium has been reached, the volume of the vessel is suddenly increased the result will be:

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Consider the equilibrium system C(s) + CO2(g) ⇔2CO(g) If C is removed, the equilibrium will _, and if CO is added, the equilibrium will _.