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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 16c
20장, 문제 16c

Indicate whether each of the following statements is true or false: (c) An oxidizing agent is needed to convert CO into CO2.

검증된 단계별 안내
1
Understand the concept of oxidation: Oxidation involves the loss of electrons or an increase in oxidation state by a molecule, atom, or ion.
Identify the oxidation states: In CO, carbon has an oxidation state of +2, and in CO2, carbon has an oxidation state of +4.
Determine the change in oxidation state: The conversion of CO to CO2 involves an increase in the oxidation state of carbon from +2 to +4.
Recognize the role of an oxidizing agent: An oxidizing agent is a substance that gains electrons and is reduced in a chemical reaction, facilitating the oxidation of another substance.
Conclude the necessity of an oxidizing agent: Since the conversion of CO to CO2 involves the oxidation of carbon, an oxidizing agent is required to accept the electrons lost by carbon.

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
3m

주요 개념

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Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, while reduction involves the gain of electrons. In the context of the question, converting carbon monoxide (CO) to carbon dioxide (CO2) involves the oxidation of CO, where it loses electrons.
추천 영상:
가이드 코스
01:53
Oxidation and Reduction Reactions

Oxidizing Agent

An oxidizing agent is a substance that facilitates oxidation by accepting electrons from another substance. In the reaction converting CO to CO2, an oxidizing agent is necessary to provide the means for CO to lose electrons and thus be oxidized. Common oxidizing agents include oxygen, chlorine, and potassium permanganate.
추천 영상:
가이드 코스
01:01
Oxidizing and Reducing Agents

Combustion Reactions

Combustion reactions are a type of chemical reaction where a substance reacts with oxygen, often producing heat and light. The conversion of CO to CO2 typically occurs during combustion processes, where CO is oxidized to CO2 in the presence of an adequate supply of oxygen, highlighting the role of oxidizing agents in these reactions.
추천 영상:
가이드 코스
02:24
Combustion Apparatus
관련 실천
교과서 질문

Indicate whether each of the following statements is true or false: (a) If something is reduced, it is formally losing electrons. (b) A reducing agent gets oxidized as it reacts.

교과서 질문

Indicate whether each of the following statements is true or false: (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

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교과서 질문

Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) PBr3(l) + 3 H2O(l) → H3PO3(aq) + 3 HBr(aq)

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교과서 질문

Indicate whether each of the following statements is true or false: (b) For the reaction Fe3+(aq) + Co2+(aq) → Fe2+(aq) + Co3+(aq), Fe3+(aq) is the reducing agent and Co2+(aq) is the oxidizing agent.

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교과서 질문

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) I2O5(s) + 5 CO(g) → I2(s) + 5 CO2(g) (b) 2 Hg2+(aq) + N2H4(aq) → 2 Hg(l) + N2(g) + 4 H+(aq) (c) 3 H2S(aq) + 2 H+(aq) + 2 NO3-(aq) → 3 S(s) + 2 NO(g) + 4 H2O(l)

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교과서 질문

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) 2 MnO4-(aq) + 3 S2-(aq + 4 H2O(l) → 3 S(s) + 2 MnO2(s) + 8 OH-(aq) (b) 4 H2O2(aq) + Cl2O7(g) + 2 OH-(aq) → 2 ClO2-(aq) + 5 H2O(l) + 4 O2(g) (c) Ba2+(aq) + 2 OH-(aq) + H2O2(aq) + 2 ClO2(aq) → Ba(ClO2)2(s) + 2 H2O(l) + O2(g)

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