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Chapter 15: Problem 67

Ozone, \(\mathrm{O}_{3}\), decomposes to molecular oxygen in the stratosphere according to the reaction \(2 \mathrm{O}_{3}(g) \rightarrow 3 \mathrm{O}_{2}(g) .\) Would an increase in pressure favor the formation of ozone or of oxygen?

Short Answer

Expert verified
An increase in pressure would favor the formation of ozone, \(\mathrm{O}_{3}\), due to the reaction seeking to counteract the change by shifting towards the side with fewer moles of gas, according to Le Chatelier's principle.

Step by step solution

01

Examine the balanced chemical equation

First, let us examine the balanced chemical equation for the decomposition reaction of ozone: \(2 \mathrm{O}_{3}(g) \rightarrow 3 \mathrm{O}_{2}(g) \) This equation tells us that 2 moles of ozone, \(\mathrm{O}_{3}\), decompose into 3 moles of molecular oxygen, \(\mathrm{O}_{2}\).
02

Analyze the reaction with respect to pressure

Now, we'll consider the effect of pressure on the reaction. If the pressure is increased, the system will react by trying to decrease the pressure, according to Le Chatelier's principle. This can be achieved by favoring the side of the reaction with fewer moles of gas. In our case, there are more moles of gas on the right side (3 moles of \(\mathrm{O}_{2}\)) than on the left side (2 moles of \(\mathrm{O}_{3}\)). Therefore, the system will favor a reaction that goes in the direction of fewer moles of gases to counteract the increased pressure.
03

Determine the favored side

Given that the system will favor the side of the reaction with fewer moles of gas when the pressure is increased, we can determine that the formation of ozone, \(\mathrm{O}_{3}\), will be favored under increased pressure. This indicates that increasing the pressure will shift the equilibrium towards the left side of the reaction, favoring formation of ozone rather than molecular oxygen. Hence, an increase in pressure would favor the formation of ozone.

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Most popular questions from this chapter

Ethene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\) reacts with halogens \(\left(\mathrm{X}_{2}\right)\) by the following reaction: $$\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{X}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{X}_{2}(g) $$ The following figures represent the concentrations at equilibrium at the same temperature when \(\mathrm{X}_{2}\) is \(\mathrm{Cl}_{2}\) (green), \(\mathrm{Br}_{2}\) (brown), and \(\mathrm{I}_{2}\) (purple). List the equilibria from smallest to largest equilibrium constant. [Section 15.3\(]\)

At \(900^{\circ} \mathrm{C}, K_{c}=0.0108\) for the reaction $$\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$$ A mixture of \(\mathrm{CaCO}_{3}, \mathrm{CaO},\) and \(\mathrm{CO}_{2}\) is placed in a \(10.0-\mathrm{L}\) vessel at \(900^{\circ} \mathrm{C}\). For the following mixtures, will the amount of \(\mathrm{CaCO}_{3}\) increase, decrease, or remain the same as the system approaches equilibrium? (a) \(15.0 \mathrm{~g} \mathrm{CaCO}_{3}, 15.0 \mathrm{~g} \mathrm{CaO},\) and \(4.25 \mathrm{~g} \mathrm{CO}_{2}\) (b) \(2.50 \mathrm{~g} \mathrm{CaCO}_{3}, 25.0 \mathrm{~g} \mathrm{CaO},\) and \(5.66 \mathrm{~g} \mathrm{CO}_{2}\) (c) \(30.5 \mathrm{~g} \mathrm{CaCO}_{3}, 25.5 \mathrm{~g} \mathrm{CaO},\) and \(6.48 \mathrm{~g} \mathrm{CO}_{2}\)

Explain why we normally exclude solvents from liquid-phase reactions in equilibrium-constant expressions.

Calculate \(K_{c}\) at \(303 \mathrm{~K}\) for \(\mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2} \mathrm{Cl}_{2}(g)\) if \(K_{p}=34.5\) at this temperature.

An equilibrium mixture of \(\mathrm{H}_{2}, \mathrm{I}_{2},\) and \(\mathrm{HI}\) at \(458{ }^{\circ} \mathrm{C}\) contains \(0.112 \mathrm{~mol} \mathrm{H}_{2}, 0.112 \mathrm{~mol} \mathrm{I}_{2},\) and \(0.775 \mathrm{~mol} \mathrm{HI}\) in a \(5.00-\mathrm{L}\) vessel. What are the equilibrium partial pressures when equilibrium is reestablished following the addition of 0.200 mol of HI?
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