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Chapter 14: Problem 54

Changes in the concentrations of the reactants and products at equilibrium have no effect on the value of the equilibrium constant. Explain this statement.

Short Answer

Expert verified
Changes in concentrations of reactants or products at equilibrium shift the equilibrium position but do not change the equilibrium constant. This is because the equilibrium constant is a measure of the energies of the reactants and products, which are only affected by temperature, not by concentration.

Step by step solution

01

- Understand the concept of equilibrium constant (Kc)

In a chemical reaction equilibrium, the equilibrium constant (Kc) is the ratio of concentrations of products to reactants, each raised to a power equal to its stoichiometric coefficient. The value of the equilibrium constant only depends on the temperature, not on the concentrations of the reaction components.
02

- Grasp the idea of change in concentration

Changes in the concentrations of reactants or products simply shift the position of the equilibrium, known as Le Chatelier's principle. However, this doesn't change the equilibrium constant (Kc). If more products are added, the reaction shifts to decrease the amount of products (towards reactants), and vice versa.
03

- Reason why the equilibrium constant remains constant

The equilibrium constant remains constant despite changes in concentrations because only changes in temperature can alter the equilibrium constant. The equilibrium constant represents the energies of the reactants and products, and these energies change only with temperature, not concentration.

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Most popular questions from this chapter

Write equilibrium constant expressions for the following reactions: $$\begin{array}{l}{\text { a. } 2 \mathrm{NO}_{2}(g) \rightleftarrows \mathrm{N}_{2} \mathrm{O}_{4}(g)} \\ {\text { b. } \mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftarrows \operatorname{COCl}_{2}(g)} \\\ {\text { c. } \mathrm{AgCl}(s) \rightleftarrows \mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q)}\end{array}$$ $$\begin{array}{c}{\mathrm{d} \cdot \mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows} \\ {\mathrm \quad \quad \quad \quad \quad \quad \quad \quad\quad \quad \quad \quad \quad {H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CH}_{3} \mathrm{COO}^{-}(a q)}\end{array}$$

Develop a model that shows the concept of equilibrium. Be sure that your model includes the impact of Le Chatelier's principle on equilibrium.

Write the solubility product expressions for the following slightly soluble salts: AgI, \(\mathrm{SrSO}_{4}, \mathrm{Ag}_{2} \mathrm{CO}_{3}, \mathrm{Ag}_{2} \mathrm{S}, \mathrm{PbI}_{2}, \mathrm{AgIO}_{3}\) \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2},\) and \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\)

Four lead salts and their solubility products are as follows: \(\mathrm{PbS}, 3.0 \times 10^{-28} ; \mathrm{PbCrO}_{4}, 1.8\) \(\times 10^{-14} ; \mathrm{PbCO}_{3}, 7.4 \times 10^{-14} ;\) and \(\mathrm{PbSO}_{4}, 2.5\) \(\times 10^{-8} .\) Calculate the \(\mathrm{Pb}^{2+}\) concentration in a saturated solution of each of these salts.

In general, which reaction (forward, reverse, or neither) is favored if the value of \(K\) at a specified temperature is a. equal to 1\(?\) b. very small? c. very small?
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