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Chapter 18: Problem 48

Discuss how catalysts can make processes more energy efficient.

Short Answer

Expert verified
Catalysts play a crucial role in making processes more energy efficient by lowering the activation energy of a reaction. This allows more reactant molecules to overcome the energy barrier and participate in the reaction, leading to a faster reaction and increased energy efficiency. By reducing energy waste and increasing selectivity, catalysts contribute to a more sustainable and environmentally friendly approach in various industries, such as the Haber-Bosch process and automobile exhaust systems. Overall, the use of catalysts can lead to improved energy efficiency, reduced waste, and a lower environmental impact.

Step by step solution

01

Understanding Catalysts

Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. They do this by providing an alternative reaction pathway with a lower activation energy, which is the minimum amount of energy required for a reaction to occur. By lowering the activation energy, more reactant molecules have sufficient energy to participate in the reaction, leading to a faster reaction rate.
02

Activation Energy in Chemical Processes

The activation energy of a reaction plays a crucial role in determining the rate and energy efficiency of a process. A high activation energy means that few molecules in the reactant mix have enough energy to overcome the energy barrier, resulting in a slower reaction. On the other hand, a low activation energy allows more molecules to react, making the reaction faster and more energy efficient. This is because less energy is wasted as heat, and a higher proportion of the energy input is used to drive the reaction forward.
03

Catalysts and Energy Efficiency

Catalysts improve energy efficiency by lowering the activation energy of a reaction, making it easier for reactant molecules to overcome the energy barrier and participate in the reaction. This results in a faster reaction, which increases the energy efficiency of the process. Additionally, catalysts can also increase the selectivity of a reaction, leading to fewer side products and reduced waste, further improving efficiency.
04

Real-World Applications

Catalysts play a vital role in various industrial processes and applications. For instance, in the Haber-Bosch process (used to synthesize ammonia), an iron catalyst is used to speed up the reaction between nitrogen and hydrogen, making the process more energy efficient and economically viable. In automobile exhaust systems, catalytic converters use catalysts like platinum, palladium, and rhodium to convert harmful pollutants, such as carbon monoxide and nitrogen oxides, into less harmful substances, thereby improving fuel efficiency and reducing emissions.
05

Overall Benefits

In summary, catalysts make processes more energy efficient by providing an alternative reaction pathway with a lower activation energy, allowing more reactant molecules to participate in the reaction, increasing the reaction rate and reducing energy waste. The use of catalysts in various industries and applications can lead to improved energy efficiency, reduced waste, and a lower environmental impact.

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Most popular questions from this chapter

The Henry's law constant for \(\mathrm{CO}_{2}\) in water at \(25^{\circ} \mathrm{C}\) is \(3.1 \times 10^{-2} \mathrm{M} \mathrm{atm}^{-1}\). (a) What is the solubility of \(\mathrm{CO}_{2}\) in water at this temperature if the solution is in contact with air at normal atmospheric pressure? (b) Assume that all of this \(\mathrm{CO}_{2}\) is in the form of \(\mathrm{H}_{2} \mathrm{CO}_{3}\) produced by the reaction between \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) : $$\mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(I) \rightarrow \mathrm{H}_{2} \mathrm{CO}_{3}(a q)$$ What is the \(\mathrm{pH}\) of this solution?

In 1986 an electrical power plant in Taylorsville, Georgia, burned \(8,376,726\) tons of coal, a national record at that time. (a) Assuming that the coal was \(83 \%\) carbon and \(2.5 \%\) sulfur and that combustion was complete, calculate the number of tons of carbon dioxide and sulfur dioxide produced by the plant during the year. (b) If \(55 \%\) of the \(\mathrm{SO}_{2}\) could be removed by reaction with powdered \(\mathrm{CaO}\) to form \(\mathrm{CaSO}_{3}\), how many tons of \(\mathrm{CaSO}_{3}\) would be produced?

Why is the photodissociation of \(\mathrm{N}_{2}\) in the atmosphere relatively unimportant compared with the photodissociation of \(\mathrm{O}_{2} ?\)

(a) Write a chemical equation that describes the attack of acid rain on limestone, \(\mathrm{CaCO}_{3}\), (b) If a limestone sculpture were treated to form a surface layer of calcium sulfate, would this help to slow down the effects of acid rain? Explain.

(a) How are the boundaries between the regions of the atmosphere determined? (b) Explain why the stratosphere, which is more than 20 miles thick, has a smaller total mass than the troposphere, which is less than 10 miles thick.
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