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Ch.19 - Electrochemistry
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.19 - Electrochemistry문제 63
19장, 문제 63

Which metal cation is the best oxidizing agent? a. Pb2+ b. Cr3+ c. Fe2+ d. Sn2+

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1
Identify the definition of an oxidizing agent: An oxidizing agent is a substance that gains electrons in a redox reaction, thereby causing another substance to be oxidized.
Understand that the strength of an oxidizing agent is determined by its ability to gain electrons. The more readily a cation gains electrons, the stronger the oxidizing agent it is.
Review the standard reduction potentials for each metal cation given. The cation with the highest positive standard reduction potential is the strongest oxidizing agent because it has the greatest tendency to gain electrons.
Locate the standard reduction potentials for Pb2+, Cr3+, Fe2+, and Sn2+ in a table of standard reduction potentials.
Compare the standard reduction potentials of the cations. The cation with the highest value is the best oxidizing agent among the choices provided.

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주요 개념

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Oxidizing Agents

An oxidizing agent is a substance that gains electrons in a chemical reaction, causing another substance to be oxidized. The strength of an oxidizing agent is often determined by its reduction potential; the higher the reduction potential, the stronger the oxidizing agent. In this context, we need to compare the reduction potentials of the given metal cations to identify which one is the best oxidizing agent.
추천 영상:
가이드 코스
01:01
Oxidizing and Reducing Agents

Reduction Potential

Reduction potential is a measure of the tendency of a chemical species to acquire electrons and be reduced. It is typically expressed in volts (V) and can be found in standard reduction potential tables. A more positive reduction potential indicates a greater ability to act as an oxidizing agent. Understanding these values is crucial for determining which cation is the best oxidizer among the options provided.
추천 영상:
가이드 코스
01:10
Standard Reduction Potentials

Metal Cations and Their Oxidation States

Metal cations can exist in various oxidation states, which influence their chemical behavior, including their ability to act as oxidizing or reducing agents. For example, Pb2+, Cr3+, Fe2+, and Sn2+ each have different oxidation states that affect their electron affinity and reactivity. Recognizing the oxidation states and their implications helps in predicting the relative strength of these cations as oxidizing agents.
추천 영상:
가이드 코스
00:57
Oxidation Numbers Example
관련 실천
교과서 질문

Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. O2(g) + 2 H2O(l) + 4 Ag(s) → 4 OH–(aq) + 4 Ag+(aq) b. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)

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교과서 질문

Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO2(s) + 4 H+(aq) + Sn(s) → Pb2+(aq) + 2 H2O(l) + Sn2+(aq)

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교과서 질문

Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO2(aq) + 4 H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq) c. Cl2(g) + 2 F–(aq) → F2(g) + 2 Cl–(aq)

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교과서 질문

Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. a. 2 Fe3+(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn2+(aq) b. O2(g) + 2 H2O(l) + 2 Cu(s) → 4 OH–(aq) + 2 Cu2+(aq) c. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)

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교과서 질문

Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. b. Br2(l) + 2 Cl–(aq) → 2 Br–(aq) + Cl2(g) c. MnO2(s) + 4 H+(aq) + Cu(s) → Mn2+(aq) + 2 H2O(l) + Cu2+(aq)

845
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