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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.20 - Electrochemistry문제 52c
20장, 문제 52c

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (c) In basic solution, Cr1OH231s2 is oxidized to CrO42-1aq2 by ClO-1aq2.

검증된 단계별 안내
1
Step 1: Write the balanced redox reaction.
Step 2: Calculate the standard cell potential (E°cell) using standard reduction potentials.
Step 3: Use the Nernst equation to calculate the standard Gibbs free energy change (∆G°) at 298 K.
Step 4: Use the relationship between ∆G° and the equilibrium constant (K) to calculate K at 298 K.
Step 5: Verify the balanced equation and calculations for consistency and accuracy.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
18m

주요 개념

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

Balancing Redox Reactions

Balancing redox reactions involves ensuring that the number of atoms and the charge are equal on both sides of the equation. This process often requires identifying the oxidation and reduction half-reactions, balancing them separately, and then combining them to form a complete balanced equation. In this case, understanding the oxidation states of chromium in Cr(OH)2 and CrO4^2- is essential.
추천 영상:
가이드 코스
01:04
Balancing Basic Redox Reactions

Standard Electromotive Force (emf)

The standard electromotive force (emf) of a reaction is the voltage produced by an electrochemical cell under standard conditions. It can be calculated using the standard reduction potentials of the half-reactions involved. A positive emf indicates a spontaneous reaction, while a negative emf suggests non-spontaneity. This concept is crucial for determining the feasibility of the redox reaction in question.
추천 영상:
가이드 코스
01:10
Standard Reduction Potentials

Gibbs Free Energy and Equilibrium Constant

Gibbs free energy (∆G°) is a thermodynamic quantity that indicates the spontaneity of a reaction at constant temperature and pressure. The relationship between ∆G° and the equilibrium constant (K) is given by the equation ∆G° = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin. This relationship allows for the calculation of K from ∆G° and vice versa, providing insight into the position of equilibrium for the reaction.
추천 영상:
가이드 코스
01:51
Gibbs Free Energy of Reactions
관련 실천
교과서 질문

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion.

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교과서 질문

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (a) Aqueous iodide ion is oxidized to I21s2 by Hg22+1aq2.

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교과서 질문

Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for each of the following reactions at 298 K:

(a) Fe(s) + Ni2+(aq) → Fe2+(aq) + Ni(s)

(b) Co(s) + 2 H+(aq) → Co2+(aq) + H2(g)

(c) 10 Br-(aq) + 2 MnO4-(aq) + 16 H+(aq) → 2 Mn2+(aq) + 8 H2O(l) + 5 Br2(l)

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교과서 질문

Given the following reduction half-reactions:

Fe3+(aq) + e- → Fe2+(aq) E°red = +0.77 V

S2O62-(aq) + 4 H+(aq) + 2 e- → 2 H2SO3(aq) E°red = +0.60 V

N2O(g) + 2 H+(aq) + 2 e- → N2(g) + H2O(l) E°red = -1.77 V

VO2+(aq) + 2 H+(aq) + e- → VO2+ + H2O(l) E°red = +1.00 V

(c) Calculate the equilibrium constant K for each reaction at 298 K.

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