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Chapter 20: Problem 15

Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons. (b) For the reaction \(\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\) \(\mathrm{Co}^{3+}(a q), \mathrm{Fe}^{3+}(a q)\) is the reducing agent and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent. (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.

Short Answer

Expert verified
(a) True: In oxidation, a species loses electrons and its oxidation state increases. (b) True: In this reaction, $\mathrm{Fe}^{3+}(a q)$ is the reducing agent and $\mathrm{Co}^{2+}(a q)$ is the oxidizing agent. (c) True: If no changes in oxidation states occur, the reaction is not a redox reaction.

Step by step solution

01

Redox Reactions: Oxidation and Reduction

A redox reaction is a type of chemical reaction where the oxidation states of atoms change. In a redox reaction, one species undergoes oxidation, while the other undergoes reduction. Oxidation and reduction can be defined as follows: - Oxidation: The process in which a species loses electrons and its oxidation state increases. - Reduction: The process in which a species gains electrons and its oxidation state decreases. A redox reaction involves a transfer of electrons between two species.
02

Oxidizing Agents and Reducing Agents

The species that gains electrons is the oxidizing agent, and the species that loses electrons is the reducing agent. The oxidizing agent causes another species to be oxidized and itself undergoes reduction. The reducing agent causes another species to be reduced and itself undergoes oxidation. Now, let's determine whether the given statements are true or false.
03

Statement (a)

If something is oxidized, it is formally losing electrons. This statement is true. When a species is undergoing oxidation, it is losing electrons and its oxidation state increases.
04

Statement (b)

For the reaction $\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\( \)\mathrm{Co}^{3+}(a q), \mathrm{Fe}^{3+}(a q)\( is the reducing agent and \)\mathrm{Co}^{2+}(a q)$ is the oxidizing agent. In this reaction, \(\mathrm{Fe}^{3+}(a q)\) is reduced to \(\mathrm{Fe}^{2+}(a q)\) because its oxidation state decreases from +3 to +2. At the same time, \(\mathrm{Co}^{2+}(a q)\) is oxidized to \(\mathrm{Co}^{3+}(a q)\), as its oxidation state increases from +2 to +3. Therefore, \(\mathrm{Fe}^{3+}(a q)\) is the reducing agent because it undergoes reduction, and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent because it undergoes oxidation. This statement is also true.
05

Statement (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. This statement is true. A redox reaction requires a change in the oxidation states of the species involved. If there are no changes in the oxidation states during a reaction, it cannot be considered a redox reaction. To summarize, Statement (a) is True. Statement (b) is True. Statement (c) is True.

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Most popular questions from this chapter

A voltaic cell utilizes the following reaction: $$ 2 \mathrm{Fe}^{3+}(a q)+\mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{Fe}^{2+}(a q)+2 \mathrm{H}^{+}(a q) $$ (a) What is the emf of this cell under standard conditions? (b) What is the emf for this cell when \(\left[\mathrm{Fe}^{3+}\right]=3.50 M, P_{\mathrm{H}_{2}}=\) \(0.95 \mathrm{atm},\left[\mathrm{Fe}^{2+}\right]=0.0010 M,\) and the \(\mathrm{pH}\) in both half-cells is 4.00\(?\)

Some years ago a unique proposal was made to raise the Titanic. The plan involved placing pontoons within the ship using a surface-controlled submarine-type vessel. The pontoons would contain cathodes and would be filled with hydrogen gas formed by the electrolysis of water. It has been estimated that it would require about \(7 \times 10^{8}\) mol of \(\mathrm{H}_{2}\) to provide the buoyancy to lift the ship (J. Chem. Educ., \(1973,\) Vol. \(50,61 )\) . (a) How many coulombs of electrical charge would be required? (b) What is the minimum voltage required to generate \(\mathrm{H}_{2}\) and \(\mathrm{O}_{2}\) if the pressure on the gases at the depth of the wreckage \((2\) \(\mathrm{mi}\) is 300 \(\mathrm{atm} ?(\mathbf{c})\) What is the minimum electrical energy required to raise the Titanic by electrolysis? (d) What is the minimum cost of the electrical energy required to generate the necessary \(\mathrm{H}_{2}\) if the electricity costs 85 cents per kilowatt-hour to generate at the site?

During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery. (a) What mass of \(\mathrm{MnO}_{2}\) is reduced at the cathode during this discharge? (b) How many coulombs of electrical charge are transferred from Zn to \(\mathrm{MnO}_{2} ?\)

During a period of discharge of a lead-acid battery, 402 \(\mathrm{g}\) of Pb from the anode is converted into PbSO \(_{4}(s) .\) (a) What of Pb from the anode is converted into PbSO \(_{4}(s) .\) (a) What mass of \(\mathrm{PbO}_{2}(s)\) is reduced at the cathode during this same period? (b) How many coulombs of electrical charge are transferred from Pb to PbO \(_{2} ?\)

A voltaic cell is constructed with all reactants and products in their standard states. Will the concentration of the reactants increase, decrease, or remain the same as the cell operates?
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