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Chapter 20: Problem 32

(a) Which electrode of a voltaic cell, the cathode or the anode, corresponds to the higher potential energy for the electrons? (b) What are the units for electrical potential? How does this unit relate to energy expressed in joules?

Short Answer

Expert verified
(a) In a voltaic cell, the anode has higher potential energy for electrons as oxidation occurs at the anode and electrons flow towards the cathode. (b) The unit for electrical potential is the volt (V). The relationship between electrical potential and energy (in joules) can be expressed as: \(1\,V = 1\,J/C\), where V represents volts, J represents joules, and C represents charge in coulombs.

Step by step solution

01

Identify the electrode with higher potential energy for electrons

In a voltaic cell, oxidation occurs at the anode, resulting in the generation of positive ions and the release of electrons. These electrons move through the external circuit towards the cathode, where reduction occurs. Due to the flow of electrons from the anode to cathode, the anode is considered to have more potential energy for the electrons.
02

Determine the unit for electrical potential

The unit for electrical potential is the volt (V), named after Alessandro Volta.
03

Relate electrical potential unit to energy expressed in joules

The potential energy of the electrons is converted into electrical potential energy when they move through the voltaic cell. Electrical potential can be expressed in energy terms since it is the work done per unit charge. The relationship between electrical potential (measured in volts) and energy (measured in joules) can be expressed as: \(1\,V = 1\,J/C\) Where V represents electrical potential in volts, J represents energy in joules, and C represents charge in coulombs. In other words, an electrical potential of 1 volt is equal to 1 joule of energy per coulomb of charge.

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Most popular questions from this chapter

A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction: $$ \operatorname{AgCl}(s)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)+\mathrm{Cl}^{-}(a q) $$ The two half-cells have \(\left[\mathrm{Cl}^{-}\right]=0.0150 \mathrm{M}\) and \(\left[\mathrm{Cl}^{-}\right]=\) \(2.55 \mathrm{M},\) respectively. (a) Which electrode is the cathode of the cell? (b) What is the standard emf of the cell? (c) What is the cell emf for the concentrations given? (d) For each electrode, predict whether \(\left[\mathrm{Cl}^{-}\right]\) will increase, decrease, or stay the same as the cell operates.

(a) Suppose that an alkaline battery was manufactured using cadmium metal rather than zinc. What effect would this have on the cell emf? (b) What environmental advantage is provided by the use of nickel-metal hydride batteries over nickel-cadmium batteries?

A voltaic cell is constructed that uses the following half-cell reactions: $$ \begin{array}{c}{\mathrm{Cu}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{Cu}(s)} \\ {\mathrm{I}_{2}(s)+2 \mathrm{e}^{-} \quad \longrightarrow 2 \mathrm{I}^{-}(a q)}\end{array} $$ The cell is operated at 298 \(\mathrm{K}\) with \(\left[\mathrm{Cu}^{+}\right]=0.25 M\) and \(\left[\mathrm{I}^{-}\right]=0.035 \mathrm{M}\) (a) Determine \(E\) for the cell at these concentrations. (b) Which electrode is the anode of the cell? (c) Is the answer to part (b) the same as it would be if the cell were operated under standard conditions? (d) If \(\left[\mathrm{Cu}^{+}\right]\) were equal to \(0.15 \mathrm{M},\) at what concentration of I \(\mathrm{I}^{-}\) would the cell have zero potential?

A voltaic cell that uses the reaction $$ \mathrm{T}^{3+}(a q)+2 \mathrm{Cr}^{2+}(a q) \longrightarrow \mathrm{Tl}^{+}(a q)+2 \mathrm{Cr}^{3+}(a q) $$ has a measured standard cell potential of \(+1.19 \mathrm{V}\) . (a) Write the two half-cell reactions. (b) By using data from Appendix E, determine \(E_{\text { red }}^{\circ}\) for the reaction involving Pd. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow.

A cell has a standard cell potential of \(+0.177 \mathrm{V}\) at 298 \(\mathrm{K}\) . What is the value of the equilibrium constant for the reaction ( a ) if \(n=1 ?(\mathbf{b})\) if \(n=2 ?(\mathbf{c})\) if \(n=3 ?\)
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