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

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.

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.

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.