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Chapter 13: Problem 9

The value of the equilibrium constant \(K\) depends on which of the following (there may be more than one answer)? a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.

Short Answer

Expert verified
The value of the equilibrium constant (K) depends on the temperature of the system (c) and the nature of the reactants and products (d). It does not depend on the initial concentrations of the reactants (a) or products (b), as they only determine the position of the initial state relative to the equilibrium state. The temperature affects the value of K differently for exothermic and endothermic reactions, while the chemical identities and stoichiometry of the reactants and products determine the value of K under a given set of conditions.

Step by step solution

01

Understanding the Equilibrium Constant (K)

The equilibrium constant (K) is a value that helps us to predict the composition of a mixture at equilibrium for a given chemical reaction. For a general reaction of the form aA + bB <-> cC + dD, the equilibrium constant, K, can be written as: \(K = \frac{[C]^c [D]^d}{[A]^a [B]^b}\) where [A], [B], [C], and [D] are the molar concentrations of the species at equilibrium.
02

Evaluate Statement a

The initial concentrations of reactants (a) do not affect the value of the equilibrium constant (K). The initial concentrations only determine the position of the initial state relative to the equilibrium state, but once the reaction has reached equilibrium, the constant K remains the same.
03

Evaluate Statement b

Similarly, the initial concentrations of products (b) do not affect the value of the equilibrium constant (K). The initial concentrations of products only determine the position of the initial state with respect to the equilibrium state, but once equilibrium is reached, the value of K remains unchanged.
04

Evaluate Statement c

The temperature of the system (c) affects the value of the equilibrium constant (K). For an exothermic reaction, increasing the temperature will shift the position of equilibrium in the opposite direction, favoring the reactants, and decreasing the value of K. Conversely, for an endothermic reaction, increasing the temperature will result in a shift towards the product side, increasing the value of K. It can be inferred that the value of K depends on the temperature for a given reaction.
05

Evaluate Statement d

The nature of the reactants and products (d) determines the value of the equilibrium constant (K). Different reactions will have different equilibrium constants at the same temperature. The chemical identities and the stoichiometry of the species participating in the reaction determine the value of K under a given set of conditions. In conclusion, the value of the equilibrium constant (K) depends on: - The temperature of the system (c) - The nature of the reactants and products (d)

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Most popular questions from this chapter

Suppose a reaction has the equilibrium constant \(K=1.3 \times 10^{8}\). What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?

Nitric oxide and bromine at initial partial pressures of \(98.4\) and \(41.3\) torr, respectively, were allowed to react at \(300 . \mathrm{K}\). At equilibrium the total pressure was \(110.5\) torr. The reaction is $$ 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{NOBr}(g) $$ a. Calculate the value of \(K_{\mathrm{p}}\). b. What would be the partial pressures of all species if \(\mathrm{NO}\) and \(\mathrm{Br}_{2}\), both at an initial partial pressure of \(0.30 \mathrm{~atm}\), were allowed to come to equilibrium at this temperature?

The synthesis of ammonia gas from nitrogen gas and hydrogen gas represents a classic case in which a knowledge of kinetics and equilibrium was used to make a desired chemical reaction economically feasible. Explain how each of the following conditions helps to maximize the yield of ammonia. a. running the reaction at an elevated temperature b. removing the ammonia from the reaction mixture as it forms c. using a catalyst d. running the reaction at high pressure

An \(8.00-\mathrm{g}\) sample of \(\mathrm{SO}_{3}\) was placed in an evacuated container, where it decomposed at \(600^{\circ} \mathrm{C}\) according to the following reaction: $$ \mathrm{SO}_{3}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) $$ At equilibrium the total pressure and the density of the gaseous mixture were \(1.80 \mathrm{~atm}\) and \(1.60 \mathrm{~g} / \mathrm{L}\), respectively. Calculate \(K_{\mathrm{p}}\) for this reaction.

In which direction will the position of the equilibrium $$ 2 \mathrm{HI}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) $$ be shifted for each of the following changes? a. \(\mathrm{H}_{2}(g)\) is added. b. \(\mathrm{I}_{2}(g)\) is removed. c. \(\mathrm{HI}(g)\) is removed. d. In a rigid reaction container, some \(\operatorname{Ar}(g)\) is added. e. The volume of the container is doubled. f. The temperature is decreased (the reaction is exothermic).
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