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Chapter 14: Problem 21

What changes in conditions would favor the reactants in the following equilibrium? $$2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftarrows 2 \mathrm{SO}_{3}(g) \quad \Delta H=-198 \mathrm{kJ}$$

Short Answer

Expert verified
To favor the reactants in the given equilibrium, we can increase the concentration of products, decrease the concentration of reactants, or increase the temperature. Pressure changes and catalysts do not noticeably affect the equilibrium.

Step by step solution

01

Analyze changes in concentration

Increasing the concentration of the reactants (SO2 and O2) or decreasing the concentration of the product (SO3) will shift the equilibrium to the right, favoring the product side, as the system works to restore equilibrium. Conversely, decreasing the concentration of reactants or increasing the concentration of products will shift the equilibrium to the left, favoring the reactants.
02

Analyze changes in temperature

According to Le Chatelier's principle, if the temperature increases, the equilibrium will shift in the direction that absorbs the heat, which is the endothermic direction. Since the reaction is exothermic (as indicated by the negative \( \Delta H \)), an increase in temperature will shift the equilibrium to the left, favoring reactants. Conversely, a decrease in temperature will shift the equilibrium to the right, favoring products.
03

Analyze changes in pressure

According to Le Chatelier's principle, an increase in pressure is expected to shift the equilibrium in the direction that reduces pressure, i.e., towards the side with fewer moles of gas. In this reaction, the number of moles of gas on both sides is the same (2 moles each). Hence, changes in pressure will not affect this equilibrium significantly.
04

Evaluate the effect of a catalyst

The introduction of a catalyst would speed up both the forward and reverse reactions equally. It does not shift the position of the equilibrium; hence, it does not favor either the reactants or the products.

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Most popular questions from this chapter

A very dilute solution of silver nitrate is added dropwise to a solution that contains equal concentrations of sodium chloride and potassium bromide. What salt will precipitate first?

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$$

What are ligands?

Why must a balanced chemical equation be used when determining \(K_{e q} ?\)

What is the distinction between a static equilibrium and a dynamic equilibrium? In which class do chemical equilibria fit?
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