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Ch.5 - Thermochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.5 - ThermochemistryProblem 48c
Chapter 5, Problem 48c

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?

Verified step by step guidance
1
Identify the sign of the enthalpy change (ΔH) for the reaction. A positive ΔH indicates that the reaction is endothermic, meaning it absorbs heat from the surroundings.
Understand that thermodynamically favored reactions are generally those that release energy (exothermic reactions), where ΔH is negative, as they lead to a decrease in the system's enthalpy, making the products more stable than the reactants.
Compare the enthalpy change of the forward reaction, which is +630 kJ, indicating that it is endothermic and requires energy input to proceed.
Consider the reverse reaction, where the sign of ΔH would be negative (-630 kJ), suggesting that it is exothermic. This reaction would release energy, making it more likely to occur spontaneously under standard conditions.
Conclude that the reverse reaction, forming liquid benzene from gaseous acetylene, is more likely to be thermodynamically favored due to its exothermic nature.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Thermodynamics and Reaction Favorability

Thermodynamics is the study of energy transformations, particularly how energy changes influence the direction of chemical reactions. A reaction is thermodynamically favored if it leads to a decrease in free energy, typically indicated by a negative change in Gibbs free energy (ΔG). In this context, the forward reaction's positive enthalpy change (ΔH = +630 kJ) suggests it absorbs heat, which may affect its favorability.
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Enthalpy and Reaction Energy

Enthalpy (H) is a measure of the total energy of a thermodynamic system, including internal energy and the energy required to make room for it by displacing its environment. A positive ΔH indicates that the reaction is endothermic, meaning it requires energy input. Understanding the enthalpy change helps predict whether a reaction will proceed spontaneously under given conditions.

Entropy and Disorder

Entropy (S) is a measure of the disorder or randomness in a system. In chemical reactions, an increase in the number of gas molecules typically leads to an increase in entropy, which can favor the reaction despite a positive enthalpy change. In this case, the decomposition of liquid benzene into gaseous acetylene increases the number of gas molecules, potentially making the forward reaction more favorable from an entropy perspective.
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Related Practice
Textbook Question

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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Textbook Question

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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Textbook Question

Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of the water. Each is then lifted out and placed in separate beakers containing 1000 g of water at 10.0 °C. Object A increases the water temperature by 3.50 °C; B increases the water temperature by 2.60 °C. (a) Which object has the larger heat capacity?

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Textbook Question

Consider the combustion of liquid methanol, CH3OH(l): CH3OH(l) + 3/2 O2(g) → CO2(g) + 2 H2O(l) ΔH = -726.5 kJ (d) If the reaction were written to produce H2O(g) instead of H2O(l), would you expect the magnitude of ΔH to increase, decrease, or stay the same? Explain.

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Textbook Question

(b) The specific heat of aluminum is 0.9 J/(g - K). Calculate its molar heat capacity.

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