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Chapter 14: Problem 60

A certain reaction has a \(K_{\text {eq }}\) value of \(1.5 \times 10^{-6}\). (a) Would this be a practical reaction from which to isolate pure product? Explain your answer.

Short Answer

Expert verified
No, this reaction would not be practical for isolating pure product because the small \(K_{\text{eq}}\) value of \(1.5 \times 10^{-6}\) indicates that the reaction favors the reactants, meaning there would be a significantly higher concentration of reactants compared to products at equilibrium, resulting in a low yield of the desired product.

Step by step solution

01

Analyze the given equilibrium constant

The given reaction has an equilibrium constant, \(K_{\text{eq}}\), of \(1.5 \times 10^{-6}\). This is a small value, which implies that the reaction favors the reactants much more than the products.
02

Determine if the reaction is practical for isolating product

Since the \(K_{\text{eq}}\) value is small, it indicates that at the equilibrium position, there will be a significantly higher concentration of reactants compared to products. Therefore, this reaction would not be considered practical for isolating pure product, as it would not provide a high yield of the desired product.

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Most popular questions from this chapter

How would the value of the equilibrium constant for a one-step reaction calculated as \(k_{\mathrm{f}} / k_{\mathrm{r}}\) compare with the value calculated from the concentrations of all substances present at equilibrium?

Cooling an exothermic reaction for which \(K_{\text {eq }}\) is very low shifts the reaction to the right, so that more product is formed, but there is a trade-off. What is the downside of cooling such a reaction, as far as forming product is concerned?

In theory, all reactions are reversible, but in practice, some are not. Explain why.

Will \(K_{\text {eq }}\) for an exothermic reaction increase or decrease when the reaction mixture is (a) heated and (b) cooled? Explain your answer.

What does the "equi" portion of the word equilibrium refer to?
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