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Chapter 14: Problem 44

Why might an industrial process be operated at high temperature even though the reaction is more favorable at lower temperatures?

Short Answer

Expert verified
An industrial process might be operated at higher temperatures despite the reaction being more favorable at lower temperatures because higher temperatures can significantly speed up reaction rates to meet production demands.

Step by step solution

01

Understand the impact of temperature on reaction favorability

Reactions are said to be more favorable at lower temperatures because lower temperatures mean a system has less thermal energy and the reaction is more likely to go in the direction that absorbs energy (endothermic). However, the favorability is only one aspect of the reaction. While a reaction may be more favorable at a certain temperature, that does not mean the reaction will proceed at a large enough rate to be useful.
02

Link between temperature and reaction rates

Higher temperatures generally speed up reactions. According to the Collision Theory, an increase in temperature means the particles have more kinetic energy, therefore they move faster and collide more frequently and with more energy. As a result, the reaction rate is often faster at higher temperatures, even if it is less favorable.
03

Determine the justification for high operating temperatures

Industrial processes often need to produce products quickly to meet demand. Therefore, even though the reaction may be more favorable at lower temperatures, it might be too slow to meet production requirements. For these cases, the reaction is carried out at higher temperatures to speed up the reaction rate, despite it being less favorable thermodynamically.

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Most popular questions from this chapter

Methanol, \(\mathrm{CH}_{3} \mathrm{OH},\) can be prepared in the presence of a catalyst by the reaction of \(\mathrm{H}_{2}\) and \(\mathrm{CO}\) at high temperatures according to the following equation: $$\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftarrows \mathrm{CH}_{3} \mathrm{OH}(g)$$ What is the concentration of \(\mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})\) in moles per liter if the concentration of \(\mathrm{H}_{2}=0.080 \mathrm{mol} / \mathrm{L}\) , the concentration of \(\mathrm{CO}=0.025 \mathrm{mol} / \mathrm{L},\) and \(K_{e q}=290\) at 700 \(\mathrm{K} ?\)

When does a pressure change affect a chemical equilibrium?

What changes in conditions would favor the products in the following equilibrium? $$\mathrm{PCl}_{5}(g) \rightleftarrows \mathrm{Cl}_{2}(g)+\mathrm{PCl}_{3}(g) \quad \Delta H=88 \mathrm{kJ}$$

Give two examples of static equilibrium and two examples of dynamic equilibrium Your examples do not have to be chemical examples.

Distinguish between solubility and solubility product constant. Explain how one may be calculated from the other.
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