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Chapter 16: Problem 66

A plot of the solubility of a certain compound \(\left(\mathrm{g} / 100 \mathrm{~g} \mathrm{H}_{2} \mathrm{O}\right)\) against temperature \(\left({ }^{\circ} \mathrm{C}\right)\) is a straight line with a positive slope. Is dissolving that compound an exothermic process?

Short Answer

Expert verified
Explain your reasoning. Answer: No, the solubility plot suggests that dissolving the compound is not an exothermic process because the solubility increases with increasing temperature, as indicated by the positive slope. In an exothermic process, the solubility would decrease with increasing temperature due to the release of heat.

Step by step solution

01

Understanding Positive Slope Relationship

A straight line with a positive slope signifies that as the temperature increases, so does the solubility of the compound in water. This means that the compound becomes more soluble.
02

Analyzing the Relationship with Exothermic Processes

In an exothermic process, heat is released when the compound dissolves, which should result in a decrease in solubility as the temperature increases. However, the given plot shows that the solubility of the compound increases with increasing temperature, which suggests that this process is not exothermic.
03

Conclusion

Since the solubility of the given compound increases with the increasing temperature, as shown by the positive slope of the solubility plot, dissolving the compound is not an exothermic process.

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