Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

(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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

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 \(25^{\circ} \mathrm{C}\) .

A voltaic cell is constructed with all reactants and products in their standard states. Will the concentration of the reactants increase, decrease, or remain 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?

A voltaic cell is constructed that is based on the following reaction: $$ \mathrm{Sn}^{2+}(a q)+\mathrm{Pb}(s) \longrightarrow \mathrm{Sn}(s)+\mathrm{Pb}^{2+}(a q) $$ (a) If the concentration of \(\mathrm{Sn}^{2+}\) in the cathode half-cell is 1.00\(M\) and the cell generates an emf of \(+0.22 \mathrm{V},\) what is the concentration of \(\mathrm{Pb}^{2+}\) in the anode half-cell? (b) If the anode half-cell contains \(\left[\mathrm{SO}_{4}^{2-}\right]=1.00 M\) in equilibrium with \(\mathrm{PbSO}_{4}(s),\) what is the \(K_{s p}\) of \(\mathrm{PbSO}_{4} ?\)

A common shorthand way to represent a voltaic cell is $$ \text {anode} | \text {anode solution} | | \text {cathode solution} | \text {cathode} $$ A double vertical line represents a salt bridge or a porous barrier. A single vertical line represents a change in phase, such as from solid to solution. (a) Write the half-reactions and overall cell reaction represented by Fel Fe \(^{2+} \| \operatorname{Ag}^{+} | A g;\) calculate the standard cell emf using data in Appendix E. (b) Write the half-reactions and overall cell reaction represented by Zn \(\left|Z \mathrm{n}^{2+}\right| \mathrm{H}^{+} | \mathrm{H}_{2} ;\) calculate the standard cell emf using data in Appendix E and use Pt for the hydrogen electrode. (c) Using the notation just described, represent a cell based on the following reaction: $$ \begin{aligned} \mathrm{ClO}_{3}^{-}(a q)+3 \mathrm{Cu}(s)+6 \mathrm{H}^{+}(a q) & \\ \longrightarrow & \mathrm{Cl}^{-}(a q)+3 \mathrm{Cu}^{2+}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l) \end{aligned} $$ Pt is used as an inert electrode in contact with the ClO \(_{3}^{-}\) and \(\mathrm{Cl}^{-} .\) Calculate the standard cell emf given: \(\mathrm{ClO}_{3}^{-}(a q)+\) \(6 \mathrm{H}^{+}(a q)+6 \mathrm{e}^{-} \longrightarrow \mathrm{Cl}^{-}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l); E^{\circ}=1.45 \mathrm{V}\).

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free