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Ch.5 - Thermochemistry
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 15th EditionCh.5 - Thermochemistry문제 48a
5장, 문제 48a

Consider the decomposition of liquid benzene, C6H6(l), to gaseous acetylene, C2H2(g): C6H6(l) → 3 C2H2(g) ΔH = +630 kJ (a) What is the enthalpy change for the reverse reaction?

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1
Identify the forward reaction and its enthalpy change: The decomposition of liquid benzene (C6H6(l)) into gaseous acetylene (C2H2(g)) has an enthalpy change (ΔH) of +630 kJ.
Understand the concept of enthalpy change for reverse reactions: The enthalpy change for the reverse reaction is equal in magnitude but opposite in sign to the enthalpy change of the forward reaction.
Write the equation for the reverse reaction: 3 C2H2(g) → C6H6(l).
Determine the sign of ΔH for the reverse reaction: Since the forward reaction is endothermic (+630 kJ), the reverse reaction will be exothermic, which means ΔH will be negative.
Calculate the magnitude of ΔH for the reverse reaction: It will be -630 kJ, indicating that energy is released when acetylene converts back to benzene.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Enthalpy Change

Enthalpy change (ΔH) is a measure of the heat content of a system at constant pressure. It indicates whether a reaction is exothermic (releases heat, ΔH < 0) or endothermic (absorbs heat, ΔH > 0). In the given reaction, the positive ΔH value of +630 kJ signifies that the decomposition of benzene into acetylene requires energy input.
추천 영상:
가이드 코스
02:34
Enthalpy of Formation

Reverse Reaction

The reverse reaction is simply the process of converting products back into reactants. According to the principle of conservation of energy, the enthalpy change for the reverse reaction is equal in magnitude but opposite in sign to that of the forward reaction. Therefore, if the forward reaction has a ΔH of +630 kJ, the reverse reaction will have a ΔH of -630 kJ.
추천 영상:
가이드 코스
03:42
Reversible Changes in Matter

Thermodynamic Principles

Thermodynamic principles govern the relationships between heat, work, and energy in chemical reactions. These principles help predict how energy is transferred during reactions. Understanding these principles is crucial for calculating enthalpy changes and determining the feasibility of reactions under different conditions.
추천 영상:
가이드 코스
01:18
First Law of Thermodynamics
관련 실천
교과서 질문

Consider the decomposition of liquid benzene, C6H6(l), to gaseous acetylene, C2H2(g): C6H6(l) → 3 C2H2(g) ΔH = +630 kJ (c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction?

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교과서 질문

Consider the decomposition of liquid benzene, C6H6(l), to gaseous acetylene, C2H2(g): C6H6(l) → 3 C2H2(g) ΔH = +630 kJ (b) What is H for the formation of 1 mol of acetylene?

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교과서 질문

Consider the combustion of isopropanol, C3H7OH(l), which is the primary component of rubbing alcohol: C3H7OH(l) + 9/2 O2(g) → 3 CO2(g) + 4 H2O(l) ΔH = -2248 kJ (b) Balance the forward reaction with whole-number coefficients. What is ΔH for the reaction represented by this equation?

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교과서 질문

At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO3: 2 KClO3(s) → 2 KCl(s) + 3 O2(g) ΔH = -89.4 kJ c. Now consider the reverse reaction, in which KClO3 is formed from KCl and O2. What is Δ𝐻 for the formation of 19.1 g KClO3 from KCl and O2?

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교과서 질문

Consider the decomposition of liquid benzene, C6H6(l), to gaseous acetylene, C2H2(g): C6H6(l) → 3 C2H2(g) ΔH = +630 kJ (d) If C6H6(g) were consumed instead of C6H6(l), would you expect the magnitude of ΔH to increase, decrease, or stay the same? Explain.

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교과서 질문

Consider the combustion of isopropanol, C3H7OH(l), which is the primary component of rubbing alcohol: C3H7OH(l) + 9/2 O2(g) → 3 CO2(g) + 4 H2O(l) ΔH = -2248 kJ a. What is the enthalpy change for the reverse reaction?

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