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Chapter 20: Problem 27

Indicate whether each statement is true or false: (a) The cathode is the electrode at which oxidation takes place. (b) A galvanic cell is another name for a voltaic cell. (c) Electrons flow spontaneously from anode to cathode in a voltaic cell.

Short Answer

Expert verified
(a) False, as cathode is the electrode where reduction occurs, not oxidation. (b) True, since galvanic cells and voltaic cells are the same and the terms can be used interchangeably. (c) True, as electrons flow spontaneously from the anode to the cathode in a voltaic cell due to the redox reaction.

Step by step solution

01

Understanding Cathode and Oxidation

In electrochemical cells, cathode is the electrode where reduction takes place, and anode is the electrode where oxidation occurs. Oxidation involves the loss of electrons, while reduction involves the gain of electrons. Now let's analyze the statement: (a) The cathode is the electrode at which oxidation takes place.
02

Verifying Statement (a)

Since we know that the cathode is where reduction occurs and not oxidation, the statement is false. #Statement b#
03

Understanding Galvanic Cells and Voltaic Cells

Galvanic cells and voltaic cells are names for the same type of electrochemical cell. These cells convert chemical energy into electrical energy through spontaneous redox reactions. The terms are used interchangeably. Now let's analyze the statement: (b) A galvanic cell is another name for a voltaic cell.
04

Verifying Statement (b)

Since galvanic cells and voltaic cells are the same and can be used interchangeably, the statement is true. #Statement c#
05

Understanding Electron Flow in Voltaic Cells

In a voltaic cell, the anode is where oxidation occurs, and the cathode is where reduction occurs. During the redox reaction, electrons are released at the anode (oxidation) and flow to the cathode (reduction) through an external circuit, generating an electric current. Now let's analyze the statement: (c) Electrons flow spontaneously from anode to cathode in a voltaic cell.
06

Verifying Statement (c)

Since electrons do flow spontaneously from the anode to the cathode in a voltaic cell due to the redox reaction, the statement is true.

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Most popular questions from this chapter

Li-ion batteries used in automobiles typically use a LiMn_ \(_{2} \mathrm{O}_{4}\) cathode in place of the LiCoO \(_{2}\) cathode found in most Li- ion batteries. (a) Calculate the mass percent lithium in each electrode material. (b) Which material has a higher percentage of lithium? Does this help to explain why batteries made with \(\mathrm{LiMn}_{2} \mathrm{O}_{4}\) cathodes deliver less power on discharging? (c) In a battery that uses a LiCoO\(_{2}\) cathode, approximately 50\(\%\) of the lithium migrates from the cathode to the anode on charging. In a battery that uses a LiMn_ \(_{2} \mathrm{O}_{4}\) cathode, what fraction of the lithium in LiMn_ \(_{2} \mathrm{O}_{4}\) would need to migrate out of the cathode to deliver the same amount of lithium to the graphite anode?

Metallic gold is collected from below the anode when a mixture of copper and gold metals is refined by electrolysis. Explain this behavior.

Indicate whether each of the following statements is true or false: (a) If something is reduced, it is formally losing electrons. (b) A reducing agent gets oxidized as it reacts. (c) An oxidizing agent is needed to convert CO into \(\mathrm{CO}_{2}\) .

Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for each of the following reactions at \(298 \mathrm{K} :\) $$ \begin{array}{l}{\text { (a) } \mathrm{Fe}(s)+\mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{Ni}(s)} \\ {\text { (b) } \mathrm{Co}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Co}^{2+}(a q)+\mathrm{H}_{2}(g)} \\ {\text { (c) } 10 \mathrm{Br}^{-}(a q)+2 \mathrm{MnO}_{4}^{-}(a q)+16 \mathrm{H}^{+}(a q) \rightarrow} \\ {\quad 2 \mathrm{Mn}^{2+}(a q)+8 \mathrm{H}_{2} \mathrm{O}(l)+5 \mathrm{Br}_{2}(l)}\end{array} $$

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