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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.15 - Chemical EquilibriumProblema 8b
Capitolo 15, Problema 8b

When lead(IV) oxide is heated above 300°C, it decomposes according to the reaction, 2 PbO2(𝑠)⇌2PbO(𝑠)+O2(𝑔). Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400°C and allowed to come to equilibrium, which of the following statements is or are true?
b. The solid left at the bottom of each vessel will be a mixture of PbO2(𝑠) and PbO(𝑠).

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Identify the chemical reaction involved: The decomposition of lead(IV) oxide (PbO2) into lead(II) oxide (PbO) and oxygen gas (O2) is given by the equation: 2 PbO2(s) ⇌ 2 PbO(s) + O2(g).
Understand the concept of equilibrium: At equilibrium, the rate of the forward reaction (decomposition of PbO2) equals the rate of the reverse reaction (formation of PbO2 from PbO and O2).
Consider the conditions: Both vessels are heated to 400°C, which is above the decomposition temperature of PbO2, allowing the reaction to proceed until equilibrium is reached.
Analyze the composition of the solid phase: At equilibrium, the solid phase will consist of both reactant (PbO2) and product (PbO) because the reaction does not go to completion and some PbO2 will remain.
Conclude about the statement: Since the reaction reaches equilibrium and both PbO2 and PbO are present in the solid phase, the statement that the solid left at the bottom of each vessel will be a mixture of PbO2(s) and PbO(s) is true.

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Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the context of the given reaction, as PbO2 decomposes into PbO and O2, the system will reach a point where the formation of PbO and O2 balances with the decomposition of PbO back into PbO2, leading to a dynamic but stable state.
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Chemical Equilibrium Concepts

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. In this case, heating the PbO2 will shift the equilibrium position to favor the formation of PbO and O2, indicating that the solid left will contain both PbO2 and PbO.
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Le Chatelier's Principle

Decomposition Reactions

Decomposition reactions involve the breakdown of a compound into simpler substances, often requiring heat or energy. The reaction of PbO2 decomposing into PbO and O2 is a classic example, where the application of heat above 300°C initiates the breakdown, leading to the formation of different solid products and gaseous oxygen, which is crucial for understanding the composition of the solids in the vessels.
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When lead(IV) oxide is heated above 300°C, it decomposes according to the reaction, 2 PbO2(𝑠) ⇌ 2PbO(𝑠) + O2(𝑔). Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400°C and allowed to come to equilibrium, which of the following statements is or are true? a. There will be less PbO2 remaining in vessel A than in vessel B.

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When lead(IV) oxide is heated above 300°C, it decomposes according to the reaction, 2 PbO2(𝑠)⇌2PbO(𝑠)+O2(𝑔). Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400°C and allowed to come to equilibrium, which of the following statements is or are true? c. The partial pressure of O2(𝑔) will be the same in vessels A and B. [Section 15.4]

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