/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 82 (a) What is the difference betwe... [FREE SOLUTION] | 91影视

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Chapter 20: Problem 82

(a) What is the difference between a battery and a fuel cell? (b) Can the "fuel" of a fuel cell be a solid?

Short Answer

Expert verified
a) The difference between a battery and a fuel cell is that a battery stores electrical energy in the form of chemical energy, while a fuel cell generates electricity by converting the chemical energy from an external fuel source. b) Yes, the fuel of a fuel cell can be a solid, especially in the case of solid oxide fuel cells that use solid fuels like metal alloys or ceramics.

Step by step solution

01

(Step 1: Understanding batteries and fuel cells)

To differentiate between a battery and a fuel cell, we need to first understand what each of them is. A battery is a device that stores electrical energy in the form of chemical energy and converts it into electricity when connected to an external circuit. On the other hand, a fuel cell is an electrochemical device that converts the chemical energy from a fuel directly into electricity and heat through a chemical reaction.
02

(Step 2: Identifying the main difference between batteries and fuel cells)

The primary difference between a battery and a fuel cell lies in how their energy is stored and generated. In a battery, the energy is stored within the device and is released by chemical reactions within the battery itself. In contrast, a fuel cell generates electricity by utilizing the energy from an external source, typically in the form of a fuel like hydrogen or methanol.
03

(Step 3: Addressing the possibility of solid fuel in fuel cells)

To answer the second question, we need to consider the nature of fuel cells and their fuel types. Most fuel cells rely on a continuous supply of fuel (typically in the form of hydrogen gas) and an oxidant (typically air) to generate electricity. However, certain types of fuel cells, like solid oxide fuel cells (SOFCs), can use solid fuels as well. These solid fuels are typically metal alloys or ceramics that contain the fuel source within their structure. So, yes, the "fuel" of a fuel cell can be a solid. In conclusion:
04

a) The difference between a battery and a fuel cell:

A battery stores electrical energy in the form of chemical energy, while a fuel cell generates electricity by converting the chemical energy from an external fuel source.
05

b) Can the "fuel" of a fuel cell be a solid?

Yes, the fuel of a fuel cell can be a solid, especially in the case of solid oxide fuel cells that use solid fuels like metal alloys or ceramics.

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Most popular questions from this chapter

A voltaic cell is based on \(\mathrm{Ag}^{+}(a q) / \mathrm{Ag}(s)\) and \(\mathrm{Fe}^{3+}(a q) /\) \(\mathrm{Fe}^{2+}(a q)\) half-cells. (a) What is the standard emf of the cell? (b) Which reaction occurs at the cathode and which at the anode of the cell? (c) Use \(S^{\circ}\) values in Appendix \(\mathrm{C}\) and the relationship between cell potential and free-energy change to predict whether the standard cell potential increases or decreases when the temperature is raised above \(25^{\circ} \mathrm{C}\) .

Is each of the following substances likely to serve as an oxidant or a reductant: (a) \(\mathrm{Ce}^{3+}(a q),\)(b) \(\mathrm{Ca}(s),\) (c) \(\mathrm{ClO}_{3}(a q)\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5}(g) ?\)

(a) Calculate the mass of Li formed by electrolysis of molten LiCl by a current of \(7.5 \times 10^{4}\) A flowing for a period of 24 \(\mathrm{h} .\) Assume the electrolytic cell is 85\(\%\) efficient. (b) What is the minimum voltage required to drive the reaction?

A voltaic cell utilizes the following reaction: $$ 4 \mathrm{Fe}^{2+}(a q)+\mathrm{O}_{2}(g)+4 \mathrm{H}^{+}(a q) \longrightarrow 4 \mathrm{Fe}^{3+}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when \(\left[\mathrm{Fe}^{2+}\right]=1.3 \mathrm{M},\left[\mathrm{Fe}^{3+}\right]=\) \(0.010 \mathrm{M}, P_{\mathrm{O}_{2}}=0.50 \mathrm{atm}\) , and the \(\mathrm{pH}\) of the solution in the cathode half-cell is 3.50\(?\)

(a) What is meant by the term reduction? (b) On which side of a reduction half-reaction do the electrons appear? (c) What is meant by the term reductant? (d) What is meant by the term reducing agent?
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