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Chapter 6: Problem 22

Explain the advantages and disadvantages of hydrogen as an alternative fuel.

Short Answer

Expert verified
Hydrogen fuel has several advantages, such as its abundance, clean emissions, and efficiency. These attributes make it an eco-friendly and effective energy source. However, disadvantages include energy-intensive production processes, complex storage and distribution, and high costs, which hinder its widespread adoption.

Step by step solution

01

Introduction to Hydrogen Fuel

Hydrogen is an alternative fuel source that has gained considerable attention in recent years. It is considered a clean energy option, as it produces water as its only byproduct, making it an environmentally friendly choice. In this exercise, we will examine the advantages and disadvantages of hydrogen as a fuel source.
02

Advantage 1: Abundance of Hydrogen

One significant advantage of hydrogen as an alternative fuel source is its abundance. Hydrogen is the most abundant element in the universe. Although hydrogen is not freely available in nature, it can be extracted from water molecules (H鈧侽) and hydrocarbon fuels (like natural gas). This means that hydrogen fuel has the potential to be virtually inexhaustible.
03

Advantage 2: Clean Emission

Hydrogen fuel cells emit only water vapor and heat as byproducts, making hydrogen an eco-friendly alternative to fossil fuels. This clean emission is a primary advantage of using hydrogen. By reducing air pollution, hydrogen fuel can lead to improved air quality and a decrease in greenhouse gas emissions.
04

Advantage 3: Efficiency

Hydrogen fuel cells are generally more efficient than internal combustion engines, allowing for more effective energy production per unit of fuel. This efficiency could lead to a decrease in energy consumption, further reducing the environmental impact and making hydrogen fuel a more economically viable option.
05

Disadvantage 1: Production and Extraction

One notable disadvantage of hydrogen fuel is that its production and extraction processes require significant amounts of energy. Currently, the primary production methods, such as steam reforming and electrolysis, often rely on fossil fuels. This causes an increase in carbon emissions and undermines the environmental advantages of using hydrogen as a fuel source.
06

Disadvantage 2: Storage and Distribution

Storing and distributing hydrogen is much more complex and challenging than traditional fossil fuels. Hydrogen has a low energy density, requiring storage in high-pressure tanks or extremely low temperatures. Additionally, the hydrogen fuel infrastructure is limited, which complicates widespread adoption of this alternative fuel.
07

Disadvantage 3: Cost

Hydrogen fuel production and storage are still relatively expensive compared to conventional fuels. This higher cost can deter consumers and limit the expansion of hydrogen fuel as a popular alternative. While technological advancements and economies of scale might help decrease costs over time, they remain a key disadvantage in the present. In conclusion, hydrogen fuel offers several advantages, including abundance, clean emissions, and efficiency, making it an attractive alternative to conventional fossil fuels. However, the challenges of production, storage, distribution, and cost continue to pose significant obstacles to widespread adoption.

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Most popular questions from this chapter

A coffee-cup calorimeter initially contains \(125 \mathrm{~g}\) water at \(24.2^{\circ} \mathrm{C}\). Potassium bromide \((10.5 \mathrm{~g})\), also at \(24.2^{\circ} \mathrm{C}\), is added to the water, and after the KBr dissolves, the final temperature is \(21.1^{\circ} \mathrm{C}\). Calculate the enthalpy change for dissolving the salt in \(\mathrm{J} / \mathrm{g}\) and \(\mathrm{kJ} / \mathrm{mol}\). Assume that the specific heat capacity of the solution is \(4.18 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}\) and that no heat is transferred to the surroundings or to the calorimeter.

The overall reaction in a commercial heat pack can be represented as $$ 4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \quad \Delta H=-1652 \mathrm{~kJ} $$ a. How much heat is released when \(4.00 \mathrm{~mol}\) iron is reacted with excess \(\mathrm{O}_{2}\) ? b. How much heat is released when \(1.00 \mathrm{~mol} \mathrm{Fe}_{2} \mathrm{O}_{3}\) is produced? c. How much heat is released when \(1.00 \mathrm{~g}\) iron is reacted with excess \(\mathrm{O}_{2} ?\) d. How much heat is released when \(10.0 \mathrm{~g} \mathrm{Fe}\) and \(2.00 \mathrm{~g} \mathrm{O}_{2}\) are reacted?

It takes \(585 \mathrm{~J}\) of energy to raise the temperature of \(125.6 \mathrm{~g}\) mercury from \(20.0^{\circ} \mathrm{C}\) to \(53.5^{\circ} \mathrm{C}\). Calculate the specific heat capacity and the molar heat capacity of mercury.

Given the following data $$ \begin{aligned} 2 \mathrm{ClF}(g)+\mathrm{O}_{2}(g) & \longrightarrow \mathrm{Cl}_{2} \mathrm{O}(g)+\mathrm{F}_{2} \mathrm{O}(g) & \Delta H &=167.4 \mathrm{~kJ} \\ 2 \mathrm{ClF}_{3}(g)+2 \mathrm{O}_{2}(g) & \longrightarrow \mathrm{Cl}_{2} \mathrm{O}(g)+3 \mathrm{~F}_{2} \mathrm{O}(g) & \Delta H &=341.4 \mathrm{~kJ} \\\ 2 \mathrm{~F}_{2}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{~F}_{2} \mathrm{O}(g) & \Delta H &=-43.4 \mathrm{~kJ} \end{aligned} $$ calculate \(\Delta H\) for the reaction $$ \mathrm{ClF}(g)+\mathrm{F}_{2}(g) \longrightarrow \mathrm{ClF}_{3}(g) $$

Assume that \(4.19 \times 10^{6} \mathrm{~kJ}\) of energy is needed to heat a home. If this energy is derived from the combustion of methane \(\left(\mathrm{CH}_{4}\right)\), what volume of methane, measured at STP, must be burned? \(\left(\Delta H_{\text {combustion }}^{\circ}\right.\) for \(\mathrm{CH}_{4}=-891 \mathrm{~kJ} / \mathrm{mol}\) )
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