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Chapter 21: Q21.32 P (page 974)

A voltaic cell is constructed with a ${Cu/Cu}^{2 +}$ half-cell and an ${Ni/Ni}^{2 +}$ half-cell. The nickel electrode is negative.
(a) Write balanced half-reactions and the overall reaction.
(b) Diagram the cell, labeling electrodes with their charges and showing the directions of electron flow in the circuit and of cation and anion flow in the salt bridge

Short Answer

Expert verified

a) ${Ni + Cu}^{2 +} 鈫� {Ni}^{2 +} + Cu$

b)

Step by step solution

01

Given in the question are as

${Ni/Ni}^{2 +}$ Half cell
${Cu/Cu}^{2 +}$ Half cell
The nickel electrode is negative, i.e., it is an anode.

02

Determining Half-reactions that are balanced and the overall reaction

Anode: $Ni 鈫� {Ni}^{2 +} {+ 2e}^{-}$

Cathode: ${Cu}^{2 +} {+ 2e}^{-} 鈫� Cu$

Overall impression: ${Ni + Cu}^{2 +} {+ 2e}^{-} 鈫� {Ni}^{2 +} {+ 2e}^{-} + Cu$

${= Ni + Cu}^{2 +} 鈫� {Ni}^{2 +} + Cu$

03

Diagram of the cell with labelling

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Most popular questions from this chapter

To improve conductivity in the electroplating of automobile bumpers, a thin coating of copper separates the steel from a heavy coating of chromium.

What mass of $Cu$ is deposited on an automobile trim piece if plating continues for $1.25 h$ at a current of $5.0 A$ ?
If the area of the trim piece is ${50.0 cm}^{2}$ , what is the thickness of the $Cu$ coating (d of ${Cu = 8.95 g/cm}^{3}$ )?

Balance each skeleton reaction, calculate $E 掳_{cell}$ , and state whether the reaction is spontaneous:

(a)role="math" localid="1663418747793" ${Cl}_{2} {(g) + Fe}^{2 +} {(aq) Cl}^{-} {(aq) + Fe}^{3 +} (aq)$

(b)role="math" localid="1663418761168" ${Mn}^{2 +} {(aq) + Co}^{3 +} {(aq) MnO}_{2} {(s) + Co}^{2 +} (aq)[acidic]$

(c) ${AgCl(s) + NO(g) Ag(s) + Cl}^{-} {(aq) + NO}_{3}^{-} (aq)[acidic]$

A voltaic cell consists of an ${Mn/Mn}^{2 +}$ half-cell and a ${Pb/Pb}^{2 +}$ half-cell. Calculate $[{Pb}^{2 +}]$ when $[{Mn}^{2 +}]$ is1.44M and ${E^{鈭�}}_{c e l l}$ is 0.44V.

The following reactions are used in batteries:

$\begin{matrix} {I2H}_{2} {(g)+O}_{2} (g) 鈫� {2H}_{2} {O(l)E}_{cell} =1.23V \\ {IIPb(s)+PbO}_{2} {(s)+2H}_{2} {SO}_{4} (aq) 鈫� {2PbSO}_{4} {(s)+2H}_{2} {O(l)E}_{cell} =2.04V \\ {III2Na(l)+FeCl}_{2} (s) 鈫� {2NaCl(s)+Fe(s)E}_{cell} =2.35V \end{matrix}$

The reaction I is used in fuel cells, II in the automobile lead-acid battery, and III in an experimental high-temperature battery for powering electric vehicles. The aim is to obtain as much work as possible from a cell while keeping its weight to a minimum. (a) In each cell, find the moles of electrons transferred and $鈭� G$ . (b) Calculate the ratio, in kJ/g, of $w_{max}$ to mass of reactants for each of the cells. Which has the highest ratio, which is the lowest, and why? (Note: For simplicity, ignore the masses of cell components that do not appear in the cell as reactants, including electrode materials, electrolytes, separators, cell casing, wiring, etc.)

Why are E half-cell values for the oxidation and reduction of water different from E掳 half-cell values for the same processes? In an aqueous electrolytic cell, nitrate ions never react at the anode, but nitrite ions do. Explain.

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