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Chapter 18: Problem 37

Explain the differences between a primary galvanic cell-one that is not rechargeable-and a storage cell (for example, the lead storage battery), which is rechargeable.

Short Answer

Expert verified
A primary galvanic cell converts chemical energy into electrical energy through a spontaneous, non-reversible redox reaction, making it non-rechargeable. Alternatively, a storage cell, like a lead-acid battery, can perform reversible redox reactions, which allows for both the use and recharge of the cell, thus making it reusable.

Step by step solution

01

Explain Primary Galvanic Cells

Primary galvanic cells are devices that convert chemical energy into electrical energy through a spontaneous redox reaction. Once the reaction inside the cell occurs and the chemicals are used up, the cell is depleted and can't be recharged or reused. Example of these type of cells are alkaline batteries.
02

Explain Rechargeable Storage Cells

Storage cells, like the lead-acid battery, can convert chemical energy into electrical energy and vice versa. They are rechargeable as the chemical reactions that occur inside the cells are reversible. When electrical energy is fed into the storage cells from an external source, the chemicals in the cell are restored to their original state, making the cell ready for another use.
03

Compare the Two

Comparatively, the primary difference between a primary galvanic cell and a storage cell is the reusability. Galvanic cells can only be used once as their internal redox reactions are not reversible, making them non-rechargeable. On the other hand, storage cells can be used multiple times as their internal redox reactions are reversible when supplied with electrical energy, making them rechargeable.

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Most popular questions from this chapter

Which species in each pair is a better oxidizing agent under standard-state conditions: (a) \(\mathrm{Br}_{2}\) or \(\mathrm{Au}^{3+} ?\) (b) \(\mathrm{H}_{2}\) or \(\mathrm{Ag}^{+} ?\) (c) \(\mathrm{Cd}^{2+}\) or \(\mathrm{Cr}^{3+} ?\) (d) \(\mathrm{O}_{2}\) in acidic media or \(\mathrm{O}_{2}\) in basic media?

Describe the basic features of a galvanic cell. Why are the two components of the cell separated from each other?

Given that \(\begin{array}{ll}2 \mathrm{Hg}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Hg}_{2}^{2+}(a q) & E^{\circ}=0.92 \mathrm{~V} \\\ \mathrm{Hg}_{2}^{2+}(a q)+2 e^{-} \longrightarrow 2 \mathrm{Hg}(l) & E^{\circ}=0.85 \mathrm{~V}\end{array}\) calculate \(\Delta G^{\circ}\) and \(K\) for the following process at \(25^{\circ} \mathrm{C}\) : \(\mathrm{Hg}_{2}^{2+}(a q) \longrightarrow \mathrm{Hg}^{2+}(a q)+\mathrm{Hg}(l)\) (The preceding reaction is an example of a disproportionation reaction in which an element in one oxidation state is both oxidized and reduced.)

A quantity of \(0.300 \mathrm{~g}\) of copper was deposited from a CuSO solution by passing a current of 3.00 A through the solution for 304 s. Calculate the value of the Faraday constant.

Describe the electrolysis of an aqueous solution of \(\mathrm{KNO}_{3}\)
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