Compare the pros and cons of a fuel cell, such as the hydrogen-oxygen fuel cell, and a coal-fired power station for generating electricity.

Short Answer

Expert verified
In terms of environmental impact, the hydrogen-oxygen fuel cell has the advantage as its operation results in water being the only by-product, compared to the significant greenhouse gas emissions from a coal-fired power station. However, fuel cells require a steady supply of hydrogen which may be costly and could pose storage challenges. In terms of efficiency, a hydrogen fuel cell can convert around 60% of the chemical energy in hydrogen into electrical energy, which is significantly higher than the 40% efficiency typical of coal-fired power plants. However, coal power stations have been around for a longer period, are well-developed, and utilize resources that are currently abundant and cheap. Potential improvements in hydrogen storage and production technology may shift this balance in the future.

Step by step solution

01

- Describe the hydrogen-oxygen fuel cell

Explain the principles of a hydrogen-oxygen fuel cell. Detail the chemical reactions involved and the byproducts of the process. Discuss the efficiency, environmental impact, cost, and practicality of using this form to produce energy.
02

- Describe the coal-fired power station

Explain the principles of a coal-fired power station. Detail how coal is used to create steam, which spins a generator to produce electricity. Discuss the efficiency, environmental impact, cost, and practicality of using coal to produce energy.
03

- Compare the two systems

Compare the features of the hydrogen-oxygen fuel cell and the coal-fired power station. Weigh the prospects of each system in terms of their respective environment footprint, efficiency, cost, reliability, and resource availability. Consider potential future developments that may impact your comparison.

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

What is the emf of a cell consisting of a \(\mathrm{Pb}^{2+} / \mathrm{Pb}\) half-cell and a \(\mathrm{Pt} / \mathrm{H}^{+} / \mathrm{H}_{2}\) half-cell if \(\left[\mathrm{Pb}^{2+}\right]=0.10 \mathrm{M}\), \(\left[\mathrm{H}^{+}\right]=0.050 \mathrm{M},\) and \(P_{\mathrm{H}}=2.0 \mathrm{~atm} ?\)

Calculate the emf of the following concentration cell at \(25^{\circ} \mathrm{C}\) : $$\mathrm{Cu}(s)\left|\mathrm{Cu}^{2+}(0.080 M) \| \mathrm{Cu}^{2+}(1.2 M)\right| \mathrm{Cu}(s)$$

An acidified solution was electrolyzed using copper electrodes. A constant current of 1.18 A caused the anode to lose \(0.584 \mathrm{~g}\) after \(1.52 \times 10^{3} \mathrm{~s}\). (a) What is the gas produced at the cathode and what is its volume at STP? (b) Given that the charge of an electron is \(1.6022 \times 10^{-19} \mathrm{C},\) calculate Avogadro's number. Assume that copper is oxidized to \(\mathrm{Cu}^{2+}\) ions.

Calcium oxalate \(\left(\mathrm{CaC}_{2} \mathrm{O}_{4}\right)\) is insoluble in water. This property has been used to determine the amount of \(\mathrm{Ca}^{2+}\) ions in blood. The calcium oxalate isolated from blood is dissolved in acid and titrated against a standardized \(\mathrm{KMnO}_{4}\) solution as described in Problem \(18.72 .\) In one test, it is found that the calcium oxalate isolated from a 10.0 -mL sample of blood requires \(24.2 \mathrm{~mL}\) of \(9.56 \times 10^{-4} \mathrm{M} \mathrm{KMnO}_{4}\) for titration. Calculate the number of milligrams of calcium per milliliter of blood.

A \(9.00 \times 10^{2}-\mathrm{mL} 0.200 \mathrm{M} \mathrm{MgI}_{2}\) was electrolyzed. As a result, hydrogen gas was generated at the cathode and iodine was formed at the anode. The volume of hydrogen collected at \(26^{\circ} \mathrm{C}\) and \(779 \mathrm{mmHg}\) was \(1.22 \times 10^{3} \mathrm{~mL}\). (a) Calculate the charge in coulombs consumed in the process. (b) How long (in min) did the electrolysis last if a current of \(7.55 \mathrm{~A}\) was used? (c) A white precipitate was formed in the process. What was it and what was its mass in grams? Assume the volume of the solution was constant.

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