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Chapter 22: Problem 12

Give an example of hydrogen as (a) an oxidizing agent and (b) a reducing agent.

Short Answer

Expert verified
Hydrogen acts as an oxidizing agent in the reaction with lithium: \(2Li(s) + H2(g) \rightarrow 2LiH(s)\). It acts as a reducing agent in the reaction with Chlorine gas: \(H2(g) + Cl2(g) \rightarrow 2HCl(g)\).

Step by step solution

01

Understanding Oxidizing and Reducing Agents

An oxidizing agent gains electrons and an reducing agent loses electrons. In an oxidation-reduction (redox) reaction, the oxidizing agent is reduced and the reducing agent is oxidized. Therefore, to find an example of Hydrogen as an oxidizing agent, look for a reaction where it is being reduced (gaining electrons) and to find an example of it as a reducing agent, look for a reaction where it is being oxidized (losing electrons).
02

Hydrogen as an Oxidizing Agent

Hydrogen can act as an oxidizing agent when it is combined with a metal. In these situations, the hydrogen is reduced (that is, it gains an electron) and is transformed into a hydride ion (H^-). An example is its reaction with lithium. The reaction can be illustrated as: \(2Li(s) + H2(g) \rightarrow 2LiH(s)\). In this reaction, Hydrogen is acting as an oxidizing agent.
03

Hydrogen as a Reducing Agent

Hydrogen can also act as a reducing agent, especially in reactions with non-metals. In such reactions, hydrogen is oxidized (loses an electron) to form a hydrogen ion (\(H^+\)). An example of this is the reaction with Chlorine gas: \(H2(g) + Cl2(g) \rightarrow 2HCl(g)\). In this reaction, Hydrogen is acting as a reducing agent since it loses electrons and thereby oxidized.

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Most popular questions from this chapter

At \(620 \mathrm{~K}\) the vapor density of ammonium chloride relative to hydrogen \(\left(\mathrm{H}_{2}\right)\) under the same conditions of temperature and pressure is \(14.5,\) although, according to its formula mass, it should have a vapor density of \(26.8 .\) How would you account for this discrepancy?

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