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Chapter 18: Problem 86

Describe three factors limiting widespread use of cars powered by fuel cells.

Short Answer

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Short answer: Fuel cell-powered cars have the advantage of being environmentally-friendly, but their widespread use is limited by high cost, lack of fueling infrastructure, and limited range and efficiency. The high cost of fuel cell vehicles is due to the expensive fuel cells production and limited availability of affordable hydrogen fuel. Additionally, the lack of hydrogen fueling infrastructure poses an inconvenience for drivers, making it more difficult to find refueling stations. Lastly, fuel cell cars may have a limited driving range and efficiency compared to traditional or electric cars, making them less practical for some drivers.

Step by step solution

01

Introduction to fuel cell-powered cars

Fuel cell-powered cars are vehicles that use fuel cells to convert hydrogen gas and oxygen into electricity, which then powers an electric motor. Unlike gasoline-powered vehicles, fuel cell cars produce no tailpipe emissions, making them more environmentally-friendly. Despite their benefits, there are several limiting factors that have hindered their widespread use.
02

Factor 1: High cost

One of the main factors limiting the widespread use of fuel cell-powered cars is their high cost. Fuel cell vehicles are relatively expensive compared to conventional petrol or diesel cars due to the cost of producing fuel cells and the limited availability of affordable hydrogen fuel. The high cost of fuel cell vehicles may make them uncompetitive in the market, especially for consumers with a limited budget.
03

Factor 2: Lack of fueling infrastructure

Another major factor limiting the widespread use of fuel cell-powered cars is the lack of hydrogen fueling infrastructure. Since hydrogen is not as readily available as gasoline or diesel, there are fewer fueling stations for hydrogen-powered vehicles. This can make it difficult for owners of fuel cell cars to find refueling stations, limiting the practicality and convenience of driving a fuel cell-powered vehicle.
04

Factor 3: Limited range and efficiency

Finally, the range and efficiency of fuel cell vehicles are factors that may limit their widespread use. Although fuel cell vehicles are generally more energy efficient than gasoline-powered cars, they may have limited driving ranges compared to traditional cars or more advanced electric vehicles. Additionally, fuel cell vehicles typically take longer to refuel compared to a fast electric vehicle charging session, which can be a further inconvenience for drivers.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Fuel Cell Technology
Fuel cell technology is at the heart of fuel cell-powered cars. It uses a chemical reaction between hydrogen and oxygen to generate electricity. This electricity powers the car's electric motor, allowing for emission-free driving. The process involves hydrogen gas entering the fuel cell along with air, where a catalyst facilitates the reaction between hydrogen and oxygen molecules.
One of the standout features of this technology is that it only produces water vapor and heat as byproducts. This makes fuel cell cars environmentally friendly. However, the production and development of the necessary fuel cells are complex and costly.
This complexity stems from the materials needed, such as platinum for catalysts, which is expensive. Fuel cell technology continues to evolve as researchers work on alternatives to reduce costs. With advancements, fuel cell technology holds potential for more sustainable transportation in the future.
Hydrogen Fuel Infrastructure
A significant challenge for the adoption of fuel cell cars is the hydrogen fuel infrastructure. Unlike gasoline stations, which are omnipresent, hydrogen fueling stations are sparse, especially outside major urban areas.
  • The scarcity makes it difficult for fuel cell vehicle owners to refuel conveniently.
  • Setting up new hydrogen stations involves substantial investment and regulation compliance.
Building this infrastructure requires coordinated efforts between governments, private sectors, and industries. It is a chicken-and-egg problem where constructing stations only becomes viable with enough cars on the road, but more people won't buy fuel cell cars without accessible refueling options.
Efforts to expand this infrastructure include developing new technologies for hydrogen production and storage, and creating policies incentivizing the construction of new stations.
Vehicle Cost Efficiency
The cost efficiency of fuel cell vehicles is another barrier limiting their widespread adoption. Currently, these cars tend to be more expensive than traditional gasoline vehicles, primarily due to the costly materials and intricate manufacturing process.
Producing and maintaining the hydrogen fuel networks add to the overall cost as well. However, potential improvements in manufacturing processes and materials could drive down costs in the future.
  • Efforts are being made to lower the price of raw materials used, like platinum.
  • Increasing economies of scale may eventually reduce the prices as production volumes grow.
Achieving competitive pricing with traditional cars is crucial for fuel cell vehicles to become a more attractive option for everyday consumers. Until then, their market appeal may remain limited to niche markets or as part of eco-friendly fleets in corporations or government agencies.

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Most popular questions from this chapter

In the redox reaction below, how many electrons are transferred for each molecule of \(\mathrm{H}_{2} \mathrm{O}_{2}\) consumed? \(2 \mathrm{MnO}_{4}^{-}(a q)+3 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \rightarrow\) $$2 \mathrm{MnO}_{2}(s)+3 \mathrm{O}_{2}(g)+2 \mathrm{OH}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(\ell)$$

An electrochemical cell with an aqueous electrolyte is based on the reaction between \(\mathrm{Ni}^{2+}(a q)\) and \(\mathrm{Cd}(s)\) producing \(\mathrm{Ni}(s)\) and \(\mathrm{Cd}^{2+}(a q)\) a. Write half-reactions for the anode and cathode. b. Write a balanced net ionic equation describing the cell reaction. c. Draw the cell diagram.

Voltaic cells based on the following pairs of half-reactions are constructed. For each pair, write a balanced equation for the cell reaction, and identify which half-reaction takes place at each anode and cathode. a. \(\mathrm{Cd}^{2+}(a q)+2 \mathrm{e}^{-} \rightarrow \mathrm{Cd}(s)\) \(\mathrm{Ag}^{+}(a q)+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(s)\) b. \(\mathrm{AgBr}(s)+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(s)+\mathrm{Br}^{-}(a q)\) \(\mathrm{MnO}_{2}(s)+4 \mathrm{H}^{+}(a q)+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}(a q)+2 \mathrm{H}_{2} \mathrm{O}(\ell)\) c. \(\mathrm{PtCl}_{4}^{2-}(a q)+2 \mathrm{e}^{-} \rightarrow \mathrm{Pt}(s)+4 \mathrm{Cl}^{-}(a q)\) \(\mathrm{AgCl}(s)+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(s)+\mathrm{Cl}^{-}(a q)\)

The standard potential of the Cu-Zn cell reaction, $$\mathrm{Zn}(s)+\mathrm{Cu}^{2+}(a q) \rightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Cu}(s)$$ is \(1.10 \mathrm{V} .\) Would the potential of the Cu-Zn cell differ from \(1.10 \mathrm{V}\) if the concentrations of both \(\mathrm{Cu}^{2+}\) and \(\mathrm{Zn}^{2+}\) were \(0.25 M ?\)

If a piece of silver is placed in a solution in which \(\left[\mathrm{Ag}^{+}\right]=\left[\mathrm{Cu}^{2+}\right]=1.00 \mathrm{M},\) will the following reaction proceed spontaneously? $$2 \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q) \rightarrow 2 \mathrm{Ag}^{+}(a q)+\mathrm{Cu}(s)$$
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