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Chapter 18: Problem 38

Discuss the advantages and disadvantages of fuel cells over conventional power plants in producing electricity.

Short Answer

Expert verified
Fuel cells have many advantages over conventional power plants, including high efficiency, no direct emissions, and versatility. However, they also have some disadvantages such as high initial cost and requirement of pure hydrogen. On the other hand, traditional power plants can generate large amounts of power and use widely available fuels, but they contribute to pollution and are relatively inefficient.

Step by step solution

01

Understanding Fuel Cells and Conventional Power Plants

Begin by gaining a clear understanding of what fuel cells and conventional power plants are, how they work, and how they produce electricity. This can be done through textbooks or reliable online resources.
02

Advantages of Fuel Cells

Next, list and explain the advantages of fuel cells in electricity production. Some of these might include high efficiency, no direct emissions, quiet operation, and versatility in energy sources.
03

Disadvantages of Fuel Cells

Then, talk about the negatives of using fuel cells for electricity generation. These could be initial cost, requirement of pure hydrogen, limitations in temperature and pressure, etc.
04

Advantages of Conventional Power Plants

Subsequently, discuss the positives of conventional power plants. Such points could be their capability to generate large quantities of electricity, established technology, and use of widely available fuel sources.
05

Disadvantages of Conventional Power Plants

Finally, go over the negatives of conventional energy generation methods. These could include pollution, inefficiency, and the use of non-renewable resources.

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Most popular questions from this chapter

A concentration cell ceases to operate when the concentrations of the two cell compartments are equal. At this stage, is it possible to generate an emf from the cell by adjusting another parameter without changing the concentrations? Explain.

For each of the following redox reactions, (i) write the half-reactions, (ii) write a balanced equation for the whole reaction, (iii) determine in which direction the reaction will proceed spontaneously under standard-state conditions: (a) \(\mathrm{H}_{2}(g)+\mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{H}^{+}(a q)+\mathrm{Ni}(s)\) (b) \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow\) \(\quad \mathrm{Mn}^{2+}(a q)+\mathrm{Cl}_{2}(g)\) (in acid solution) \(\begin{array}{ll}\text { (c) } \mathrm{Cr}(s)+\mathrm{Zn}^{2+}(a q) & \longrightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{Zn}(s)\end{array}\)

What is the difference between a galvanic cell (such as a Daniell cell) and an electrolytic cell?

The diagram here shows an electrolytic cell consisting of a Co electrode in a \(2.0 \mathrm{M} \mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}\) solution and a Mg electrode in a \(2.0 \mathrm{M} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) solution. (a) Label the anode and cathode and show the halfcell reactions. Also label the signs \((+\) or \(-)\) on the battery terminals. (b) What is the minimum voltage to drive the reaction? (c) After the passage of \(10.0 \mathrm{~A}\) for \(2.00 \mathrm{~h}\) the battery is replaced with a voltmeter and the electrolytic cell now becomes a galvanic cell. Calculate \(E_{\text {cell. }}\) Assume volumes to remain constant at \(1.00 \mathrm{~L}\) in each compartment.

The cathode reaction in the Leclanché cell is given by $$2 \mathrm{MnO}_{2}(s)+\mathrm{Zn}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{ZnMn}_{2} \mathrm{O}_{4}(s)$$ If a Leclanché cell produces a current of \(0.0050 \mathrm{~A}\), calculate how many hours this current supply will last if there are initially \(4.0 \mathrm{~g}\) of \(\mathrm{MnO}_{2}\) present in the cell. Assume that there is an excess of \(\mathrm{Zn}^{2+}\) ions.
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