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Chapter 14: Problem 29

What do we mean by the position of a reaction's equilibrium, and what practical consequence can it have?

Short Answer

Expert verified
The position of a reaction's equilibrium refers to the state where concentrations of reactants and products remain constant over time, with the forward and reverse reaction rates being equal. The equilibrium constant (K_eq) indicates whether the position is more favorable towards products or reactants. Factors such as concentration, temperature, and pressure can affect the equilibrium position, according to Le Chatelier's principle. The practical consequence of understanding and controlling the position of equilibrium is essential, especially in industrial processes like the Haber process for ammonia production, as it helps in optimizing reaction conditions for maximum yield and efficiency.

Step by step solution

01

Definition of Equilibrium Position

Equilibrium position refers to the state of a chemical reaction where the concentrations of reactants and products remain constant over time. At this point, the forward reaction rate is equal to the reverse reaction rate. The equilibrium position can be described by the equilibrium constant (K_eq), which is a function of the concentrations of products and reactants. High equilibrium constant (K_eq) values indicate that the equilibrium position is more favorable towards the products, while low K_eq values show that the reaction lies more on the side of the reactants.
02

Factors Affecting Equilibrium Position

The equilibrium position can be influenced by several factors such as concentration of reactants and products, temperature, and pressure. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in any of these factors, the reaction will shift its equilibrium position to counteract the change. For example, if the concentration of reactants is increased, the reaction will shift towards the production of more products to re-establish equilibrium.
03

Practical Consequences of Equilibrium Position

The position of equilibrium in a chemical reaction is important, especially in industrial processes. Knowing the equilibrium position helps in optimizing the reaction conditions to yield more of the desired product. For instance, in the Haber process, which is used for ammonia production, the position of equilibrium is manipulated by adjusting the temperature, pressure, and concentration of the reactants to maximize the yield of ammonia. In this context, understanding and controlling the position of a reaction's equilibrium can have significant practical consequences in terms of efficiency and overall production yield.

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Most popular questions from this chapter

Will \(K_{\text {eq }}\) for an exothermic reaction increase or decrease when the reaction mixture is (a) heated and (b) cooled? Explain your answer.

Write the expression for \(K_{\text {eq }}\) for the reaction \(4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightleftarrows 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\)

(a) Write the equilibrium constant expression for the reaction $$ \mathrm{PbI}_{2}(s) \leftrightarrows \mathrm{Pb}^{2+}(a q)+2 \mathrm{I}^{-}(a q) $$ (b) How would the equilibrium be affected if \(\mathrm{PbI}_{2}(s)\) were added? (c) How would the equilibrium be affected if \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(s)\) were added? (Hint: Don't forget that \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) is a water-soluble salt.)

Phosphorus pentachloride gas decomposes to \(\mathrm{PCl}_{3}(\mathrm{~g})\) and \(\mathrm{Cl}_{2}(\mathrm{~g}) .\) At equilibrium, the concentrations of the decomposition products are \(5.50 \times 10^{-3} \mathrm{M}\) for \(\mathrm{PCl}_{3}(\mathrm{~g})\) and \(0.125 \mathrm{M}\) for \(\mathrm{Cl}_{2}(g)\). What is the equilibrium concentration of \(\mathrm{PCl}_{5}\) ? The equilibrium constant for this reaction is \(7.50 \times 10^{-2}\).

At \(25^{\circ} \mathrm{C}\), the solubility of calcium oxalate, \(\mathrm{CaC}_{2} \mathrm{O}_{4}\), in water is \(6.1 \mathrm{mg} / \mathrm{L}\). (a) What are the equilibrium molar concentrations of \(\mathrm{Ca}^{2+}(a q)\) and \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}(a q) ?\) (b) Calculate \(K_{\mathrm{sp}}\) for calcium oxalate.
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