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Chapter 14: Problem 14

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?

Short Answer

Expert verified
a. When the value of \(K\) is equal to 1, neither the forward nor the reverse reaction is favored. b. When the value of \(K\) is very small, the reverse reaction is favored. c. When the value of \(K\) is very large, the forward reaction is favored.

Step by step solution

01

Understanding the relation of K and reaction direction

The value of K determines whether a reaction is mostly reactants, mostly products, or somewhat equal amounts of both. If K > 1, the reaction is product favored; meaning it will proceed in the forward direction until equilibrium is reached. If K < 1, the reaction is reactant favored; meaning it will proceed in the reverse direction until equilibrium is reached.
02

Value of K equal to 1

When the equilibrium constant \(K\) equals 1, it means that the concentrations of the reactants and the products are equal at equilibrium. As such, neither the forward nor the reverse reaction is favored.
03

Value of K very small

When the equilibrium constant \(K\) is very small (K << 1), it means that at equilibrium, the concentration of the reactants is greater than that of the products. Therefore, the reverse reaction is favored.
04

Value of K very large

When the equilibrium constant \(K\) is very large (K >> 1), it means that at equilibrium, the concentration of the products is greater than that of the reactants. Therefore, the forward reaction is favored.

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Most popular questions from this chapter

Does the forward reaction rate ever equal zero? Why or why not?

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

Explain the meaning of the terms reversible reaction, completion reaction, and reaction at equilibrium.

Determine the value of the equilibrium constant for each reaction below assuming that the equilibrium concentrations are as specified. $$\text {(a.)}A+B \rightleftarrows C ;[A]=2.0 ;[B]=3.0 ;[C]=4.0$$ $$\begin{array}{l}{\text { b. } \mathrm{D}+2 \mathrm{E} \rightleftarrows \mathrm{F}+3 \mathrm{G} ;[\mathrm{D}]=1.5 ;[\mathrm{E}]=2.0} \\\ {[\mathrm{F}]=1.8 ;[\mathrm{G}]=1.2}\end{array}$$ $$\mathrm{c} \cdot \mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \rightleftarrows 2 \mathrm{NH}_{3}(\mathrm{g}) ;\left[\mathrm{N}_{2}\right]=0.45\( \)\left[\mathrm{H}_{2}\right]=0.14 ;\left[\mathrm{NH}_{3}\right]=0.62$$

An equilibrium mixture at a specific temperature is found to consist of \(1.2 \times 10^{-3}\) \(\operatorname{mol} / \mathrm{L} \mathrm{HCl}, 3.8 \times 10^{-4} \mathrm{moll} \mathrm{O}_{2}, 5.8 \times 10^{-2}\) \(\mathrm{mol} / \mathrm{L} \mathrm{H}_{2} \mathrm{O},\) and \(5.8 \times 10^{-2} \mathrm{mol} / \mathrm{L} \mathrm{Cl}_{2}\) according to the following: $$4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightleftarrows 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+2 \mathrm{Cl}_{2}(\mathrm{g})$$ Determine the value of the equilibrium constant for this system.
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