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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 - The cathode is the electrode at which reduction takes place. (b) True - A galvanic cell is another name for a voltaic cell. (c) True - Electrons flow spontaneously from anode to cathode in a voltaic cell.

Step by step solution

01

Statement (a)#

The cathode is the electrode at which oxidation takes place. This statement is false. In electrochemical cells, the cathode is the electrode where reduction takes place, while the anode is the electrode where oxidation takes place.
02

Statement (b)#

A galvanic cell is another name for a voltaic cell. This statement is true. Galvanic cells and voltaic cells are two names for the same thing. They are electrochemical cells in which a spontaneous redox reaction generates electric current. In these cells, the anode is the site of oxidation, and the cathode is the site of reduction.
03

Statement (c)#

Electrons flow spontaneously from anode to cathode in a voltaic cell. This statement is true. In a voltaic (galvanic) cell, the anode is the site of oxidation, meaning that it is losing electrons. These electrons flow through the external circuit to the cathode, which is the site of reduction and where these electrons are gained. This flow of electrons from anode to cathode generates an electric current.

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Most popular questions from this chapter

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate \(\Delta G^{\circ}\) at \(298 \mathrm{~K},\) and calculate the equilibrium constant \(K\) at \(298 \mathrm{~K}\). (a) Aqueous iodide ion is oxidized to \(\mathrm{I}_{2}(s)\) by \(\mathrm{Hg}_{2}^{2+}(a q) .\) (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion. (c) In basic solution, \(\mathrm{Cr}(\mathrm{OH})_{3}(s)\) is oxidized to \(\mathrm{CrO}_{4}^{2-}(a q)\) by \(\mathrm{ClO}^{-}(a q)\)

A voltaic cell is constructed that uses the following reaction and operates at \(298 \mathrm{~K}\) : $$ \mathrm{Zn}(s)+\mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Ni}(s) $$ (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when $\left[\mathrm{Ni}^{2+}\right]=3.00 \mathrm{M}\( and \)\left[\mathrm{Zn}^{2+}\right]=0.100 \mathrm{M} ?(\mathbf{c})$ What is the emf of the cell when \(\left[\mathrm{Ni}^{2+}\right]=0.200 M\) and \(\left[\mathrm{Zn}^{2+}\right]=0.900 \mathrm{M} ?\)

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 \(\left[\mathrm{Cl}^{-}\right]=\) \(2.55 M,\) 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) What conditions must be met for a reduction potential to be a standard reduction potential? (b) What is the standard reduction potential of a standard hydrogen electrode? (c) Why is it impossible to measure the standard reduction potential of a single half-reaction?

If the equilibrium constant for a one-electron redox reaction at $298 \mathrm{~K}\( is \)2.2 \times 10^{-5},\( calculate the corresponding \)\Delta G^{\circ}\( and \)E^{\circ}$.
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