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Chapter 19: Problem 14

Which of the following reagents can oxidize \(\mathrm{H}_{2} \mathrm{O}\) to \(\mathrm{O}_{2}(g)\) under standard-state conditions? \(\mathrm{H}^{+}(a q)\) \(\mathrm{Cl}^{-}(a q), \mathrm{Cl}_{2}(g), \mathrm{Cu}^{2+}(a q), \mathrm{Pb}^{2+}(a q), \mathrm{MnO}_{4}^{-}(a q)\) (in acid).

Short Answer

Expert verified
Only \(MnO_4^-(aq)\) in acidic solution can oxidize \(H_2O\) to \(O_2\) under standard-state conditions.

Step by step solution

01

Understand the Oxidizing Agent Concept

An oxidizing agent is a substance that has the ability to oxidize another substance, meaning it takes electrons from that other substance. In the process, the oxidizing agent itself gets reduced. The oxidizing power of a substance can be confirmed by checking its reduction potential. A higher reduction potential indicates that the substance is a good oxidizing agent.
02

Understand Standard Reduction Potentials

Standard reduction potentials are measured under standard conditions: temperature of 25°C, pressure of 1 atmosphere, and a concentration of 1 M. In this problem, we have to identify the reagent that can oxidize water to oxygen gas under standard conditions. This means we are looking for a reagent with a standard reduction potential greater than those of water and oxygen.
03

Identify Potentials and Determine the Suitable Reagent

The reduction half-reaction for water is as follows: \(O_2(g) + 4H^+ + 4e^- \rightarrow 2H_2O\) with a standard potential of 1.23V. The given reagents are \(H^+(aq)\), \(Cl^-(aq)\), \(Cl_2(g)\), \(Cu^{2+}(aq)\), \(Pb^{2+}(aq)\), and \(MnO_4^-(aq)\). Among these, only \(MnO_4^-(aq)\) has a higher standard reduction potential (+1.51V): \(MnO_4^- + 8H^+ + 5e^- \rightarrow Mn^{2+} + 4H_2O\). Therefore, only \(MnO_4^-(aq)\) in acidic solution can oxidize \(H_2O\) to \(O_2\).

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Most popular questions from this chapter

An acidified solution was electrolyzed using copper electrodes. A constant current of 1.18 A caused the anode to lose \(0.584 \mathrm{~g}\) after \(1.52 \times 10^{3} \mathrm{~s}\). (a) What is the gas produced at the cathode and what is its volume at STP? (b) Given that the charge of an electron is \(1.6022 \times 10^{-19} \mathrm{C}\), calculate Avogadro's number. Assume that copper is oxidized to \(\mathrm{Cu}^{2+}\) ions.

Consider a galvanic cell consisting of a magnesium electrode in contact with \(1.0 \mathrm{MMg}\left(\mathrm{NO}_{3}\right)_{2}\) and a cadmium electrode in contact with \(1.0 \mathrm{M} \mathrm{Cd}\left(\mathrm{NO}_{3}\right)_{2}\) Calculate \(E^{\circ}\) for the cell, and draw a diagram showing the cathode, anode, and direction of electron flow.

What is the potential of a cell made up of \(\mathrm{Zn} / \mathrm{Zn}^{2+}\) and \(\mathrm{Cu} / \mathrm{Cu}^{2+}\) half-cells at \(25^{\circ} \mathrm{C}\) if \(\left[\mathrm{Zn}^{2+}\right]=0.25 \mathrm{M}\) and \(\left[\mathrm{Cu}^{2+}\right]=0.15 \mathrm{M} ?\)

Industrially, copper is purified by electrolysis. The impure copper acts as the anode, and the cathode is made of pure copper. The electrodes are immersed in a \(\mathrm{CuSO}_{4}\) solution. During electrolysis, copper at the anode enters the solution as \(\mathrm{Cu}^{2+}\) while \(\mathrm{Cu}^{2+}\) ions are reduced at the cathode. (a) Write half-cell reactions and the overall reaction for the electrolytic process. (b) Suppose the anode was contaminated with \(\mathrm{Zn}\) and \(\mathrm{Ag} .\) Explain what happens to these impurities during electrolysis. (c) How many hours will it take to obtain \(1.00 \mathrm{~kg}\) of \(\mathrm{Cu}\) at a current of \(18.9 \mathrm{~A} ?\)

Calculate the amounts of \(\mathrm{Cu}\) and \(\mathrm{Br}_{2}\) produced in \(1.0 \mathrm{~h}\) at inert electrodes in a solution of \(\mathrm{CuBr}_{2}\) by a current of 4.50 A.
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