Open Question
(a) What is meant by the term reduction? (b) On which side of a reduction half-reaction do the electrons appear? (c) What is meant by the term reductant? (d) What is meant by the term reducing agent?
Ch.20 - Electrochemistry
Chapter 20, Problem 16c
Indicate whether each of the following statements is true or false: (c) An oxidizing agent is needed to convert CO into CO2.
Verified step by step guidance1
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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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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.
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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.
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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.
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Related Practice
Textbook Question
Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons.
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Textbook Question
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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Textbook Question
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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Textbook Question
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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Textbook Question
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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