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Chapter 5: Problem 56

In which of the following reactions does water act as an oxidising agent? (a) \(3 \mathrm{~F}_{2}+3 \mathrm{H}_{2} \mathrm{O} \longrightarrow 6 \mathrm{HF}+\mathrm{O}_{3}\) (b) \(\mathrm{CaC}_{2}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{C}_{2} \mathrm{H}_{2}\) (c) \(\quad \mathrm{C}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{CO}+\mathrm{H}_{2}\) (d) \(\mathrm{AIN}+3 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Al}(\mathrm{OH})_{3}+\mathrm{NH}_{3}\)

Short Answer

Expert verified
Reaction (c)

Step by step solution

01

Identify the Role of Water

To determine if water acts as an oxidizing agent, we need to see if water undergoes reduction. An oxidizing agent gains electrons and therefore its oxidation number decreases in the reaction.
02

Analyze Reaction (a)

In reaction \(3 \mathrm{~F}_{2}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 6\mathrm{HF}+\mathrm{O}_{3}\), water \((\mathrm{H}_2\mathrm{O})\) loses hydrogens to form \(\mathrm{HF}\) and produces \(\mathrm{O}_3\). To check the oxidation states: Oxygen typically has an oxidation state of \(-2\) in \(\mathrm{H}_2\mathrm{O}\), which changes to a neutral \(0\) state in \(\mathrm{O}_3\). This indicates an increase, meaning no reduction occurs. Hence, \(\mathrm{H}_2\mathrm{O}\) is not the oxidizing agent.
03

Analyze Reaction (b)

In reaction \(\mathrm{CaC}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{C}_{2} \mathrm{H}_{2}\), water forms \(\mathrm{Ca}(\mathrm{OH})_{2}\) and acetylene \(\mathrm{C}_{2}\mathrm{H}_2\). Oxygen maintains its \(-2\) oxidation state, and hydrogen remains at \(+1\) throughout the reaction, with no reduction of water observed. Hence, \(\mathrm{H}_2\mathrm{O}\) is not the oxidizing agent.
04

Analyze Reaction (c)

In reaction \(\mathrm{C}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{CO}+\mathrm{H}_{2}\), water \((\mathrm{H}_2\mathrm{O})\) contributes to the formation of carbon monoxide \((\mathrm{CO})\) and hydrogen gas \((\mathrm{H}_2)\). The hydrogen in water has an oxidation state change from \(+1\) in \(\mathrm{H}_2\mathrm{O}\) to \(0\) in \(\mathrm{H}_2\), indicating a gain of electrons. As such, water acts as an oxidizing agent, receiving electrons from carbon, which is oxidized from \(0\) to \(+2\) in \(\mathrm{CO}\).
05

Analyze Reaction (d)

In reaction \(\mathrm{AIN}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Al} (\mathrm{OH})_{3}+\mathrm{NH}_{3}\), water reacts to produce \(\mathrm{Al}(\mathrm{OH})_{3}\) and \(\mathrm{NH}_3\). The oxidation state of hydrogen remains \(+1\), and oxygen remains \(-2\). There is no change in oxidation states for atoms in water, indicating water is not reduced. Thus, water is not an oxidizing agent.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidation-Reduction Reactions
Oxidation-reduction reactions or redox reactions involve the transfer of electrons between substances. This electron exchange is critical in determining the chemical behavior of compounds during these reactions.
To easily identify these redox processes, keep in mind:
  • Oxidation is the loss of electrons and typically results in an increase in oxidation state.
  • Reduction is the gain of electrons and leads to a decrease in oxidation state.
  • The substance that gives away electrons is called the reducing agent, while the one that gains electrons is the oxidizing agent.
Redox reactions are vital in many chemical and biological processes, even powering batteries and cellular respiration. Spotting these electron transfers can help in understanding reaction mechanisms and energy changes.
Oxidation States
Oxidation states, also known as oxidation numbers, provide a systematic way to understand electron distribution in molecules. They are especially helpful in balancing redox reactions and identifying the roles substances play as oxidizing or reducing agents.
Some key points about oxidation states include:
  • Elements in pure form (e.g., \( \text{O}_2 \) or \( \text{H}_2 \)) have an oxidation state of zero.
  • In a compound, hydrogen usually holds an oxidation state of \(+1\), and oxygen \(-2\).
  • The sum of oxidation states in a neutral molecule must equal zero, whereas in ions, it equals the ion's charge.
Assigning these states allows for a straightforward way to track electron transfer during chemical reactions, aiding in the prediction and explanation of chemical behavior.
Chemical Reactions Analysis
Analyzing chemical reactions involves understanding the transformation of reactants into products while keeping mass and charge balanced. Such analysis helps predict reaction outcomes and identifies potential intermediates and energy changes.
Steps in a typical chemical reaction analysis include:
  • Identifying the type of reaction: is it redox, acid-base, combustion, etc.
  • Writing balanced chemical equations, ensuring atoms and charge are conserved.
  • Identifying oxidative, reductive, or spectator ions/elements.
  • Sometimes employing models like Lewis structures to visualize electron shifts.
Through these approaches, chemists can predict the behavior of unknown reactions or alter conditions to favor the formation of desired products.
Water as an Oxidizing Agent
Water can sometimes act as an oxidizing agent in chemical reactions, which means it accepts electrons from another substance. This is a special feature because water is usually perceived as stable and non-reactive.
Characteristics of water's role as an oxidizing agent include:
  • Water itself gets reduced, usually resulting in changes to its internal oxidation states.
  • It can change from \( \text{H}_2\text{O} \) to \( \text{H}_2 \), showing a reduction in its oxidation state with hydrogen moving from \(+1\) to 0.
  • This process is significant in biochemistry and energy storage systems, like hydrogen production.
Understanding when and how water can act as an oxidizing agent broadens our perspective on its reactivity and potential uses in various chemical processes.

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