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Chapter 14: Problem 51

A student wrote, "The larger the equilibrium constant, the greater the rate at which reactants convert to products." How was he wrong?

Short Answer

Expert verified
The student was wrong because the equilibrium constant provides insights into the relative quantities of reactants and products at the equilibrium state, not the rate at which reactants convert to products. A high equilibrium constant does not necessarily equate to a fast reaction rate, and vice versa.

Step by step solution

01

Understanding Concepts and Identification of the Error

Understand the concept of equilibrium constant (K) and reaction rate. The equilibrium constant describes the ratio of product concentrations to reactant concentrations at equilibrium, with each raised to the power of their stoichiometric coefficients. The reaction rate, on the other hand, expresses how quickly reactants convert to products. From these definitions, identify the error in the student's statement, which is the incorrect association of equilibrium constant with reaction rate.
02

Formulating Explanation

Commence explaining that the concept of reaction rate and equilibrium constant are separate aspects of a chemical reaction. Highlight that equilibrium constant talks about the relative quantities of reactants and products at equilibrium state, but it does not describe how quickly this state is achieved, hence, it does not relate to the reaction rate.
03

Final Statement and Explanation

Finalize the explanation by pointing out, a reaction can have a high equilibrium constant (more products at equilibrium) but may take a long time to reach this state, i.e., it could have a low reaction rate. Conversely, a reaction can also have a low equilibrium constant (more reactants at equilibrium) but can occur very swiftly - for example, in explosive reactions.

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Most popular questions from this chapter

Analysis of an equilibrium mixture in which the following equilibrium exists gave \(\left[\mathrm{OH}^{-}\right]=\left[\mathrm{HCO}_{3}^{-}\right]=3.2 \times 10^{-3} .\) $$\mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q) \rightleftarrows \mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$ The equilibrium constant is \(4.7 \times 10^{3} .\) What is the concentration of the carbonate ion?

What changes in conditions would favor the products in the following equilibrium? $$\mathrm{PCl}_{5}(g) \rightleftarrows \mathrm{Cl}_{2}(g)+\mathrm{PCl}_{3}(g) \quad \Delta H=88 \mathrm{kJ}$$

What is the change in the rate of the forward reaction after the reaction is at equilibrium?

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