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Ch.19 - Chemical Thermodynamics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.19 - Chemical Thermodynamics문제 60
19장, 문제 60

Using data from Appendix C, calculate the change in Gibbs free energy for each of the following reactions. In each case, indicate whether the reaction is spontaneous at 298 K under standard conditions.
(a) 2 Ag(s) + Cl2(g) → 2 AgCl(s)
(b) P4O10(s) + 16 H2(g) → 4 PH3(g) + 10 H2O(g)
(c) CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g)
(d) 2 H2O2(l) → 2 H2O(l) + O2(g)

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1
Identify the standard Gibbs free energy of formation (ΔG_f^°) for each reactant and product from Appendix C for each reaction.
For each reaction, use the formula ΔG_rxn^° = Σ(ΔG_f^° products) - Σ(ΔG_f^° reactants) to calculate the standard Gibbs free energy change.
For reaction (a), calculate ΔG_rxn^° using the values for Ag(s), Cl2(g), and AgCl(s).
For reaction (b), calculate ΔG_rxn^° using the values for P4O10(s), H2(g), PH3(g), and H2O(g).
Determine the spontaneity of each reaction at 298 K by checking if ΔG_rxn^° is negative (spontaneous) or positive (non-spontaneous).

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주요 개념

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Gibbs Free Energy

Gibbs free energy (G) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. It is calculated using the formula ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. A negative ΔG indicates that a reaction is spontaneous under the given conditions.
추천 영상:
가이드 코스
01:51
Gibbs Free Energy of Reactions

Standard Conditions

Standard conditions refer to a set of specific conditions used as a reference point in thermodynamics, typically defined as 1 bar of pressure and a specified temperature, usually 298 K (25°C). Under these conditions, the standard Gibbs free energy change (ΔG°) can be determined for reactions, allowing for the assessment of spontaneity and equilibrium. It is crucial to ensure that calculations are performed under these standardized conditions for consistency.
추천 영상:
가이드 코스
01:10
Standard Reduction Potentials

Spontaneity of Reactions

The spontaneity of a reaction indicates whether it can occur without external intervention. A reaction is considered spontaneous if it has a negative Gibbs free energy change (ΔG < 0) at the specified conditions. Factors influencing spontaneity include enthalpy changes (ΔH), entropy changes (ΔS), and temperature. Understanding these factors helps predict the direction of chemical reactions and their feasibility.
추천 영상:
가이드 코스
04:20
Spontaneity of Processes
관련 실천
교과서 질문

Use data in Appendix C to calculate ΔH°, ΔS°, and ΔG° at 25 °C for each of the following reactions.

a. 4 Cr(s) + 3 O2(g) → 2 Cr2O3(s)

b. BaCO3(s) → BaO(s) + CO2(g)

c. 2 P(s) + 10 HF(g) → 2 PF5(g) + 5 H2(g)

d. K(s) + O2(g) → KO2(s)

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교과서 질문

Using data from Appendix C, calculate ΔG° for the following reactions. Indicate whether each reaction is spontaneous at 298 K under standard conditions.

(a) 2 SO2(g) + O2(g) → 2 SO3(g)

(b) NO2(g) + N2O(g) → 3 NO(g)

(c) 6 Cl2(g) + 2 Fe2O3(s) → 4 FeCl3(s) + 3 O2(g)

(d) SO2(g) + 2 H2(g) → S(s) + 2 H2O(g)

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교과서 질문

Sulfur dioxide reacts with strontium oxide as follows: SO2(g) + SrO(g) → SrSO3(s) (a) Without using thermochemical data, predict whether ΔG° for this reaction is more negative or less negative than ΔH°.

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