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Chapter 1: Problem 23

When calcium chloride \(\left(\mathrm{CaCl}_{2}\right)\) dissolves in water, the temperature of the water increases dramatically. Compared to \(\mathrm{CaCl}_{2},\) what must be true regarding the hydration energy of \(\mathrm{CaF}_{2} ?\) (A) It would be greater because fluoride is smaller than chloride. (B) It would be the same because the charges of fluoride and chloride are identical. (C) It would be the same because hydration energy is only dependent on the IMFs present in water. (D) It would be smaller because the molar mass of \(\mathrm{CaF}_{2}\) is smaller than that of \(\mathrm{CaCl}_{2}\) .

Short Answer

Expert verified
(A) It would be greater because fluoride is smaller than chloride.

Step by step solution

01

Analyze the Properties of Fluoride and Chloride Ions

Fluoride is smaller than chloride. This would mean that water molecules can get closer to fluoride, which could impact the amount of energy that is released in the hydration process.
02

Compare Hydration Energies

Hydration energy is dependent on the forces between the ions and the water molecules. Because fluoride is smaller than chloride, the forces of attraction between the water molecules and the fluoride ion are stronger. Therefore, more energy is released when CaF2 dissolves than when CaCl2 dissolves.
03

Choose the Correct Answer

The greatest amount of energy is released when the smallest, most highly charged ions are hydrated. Therefore, the hydration energy of CaF2 would be greater because fluoride is smaller than chloride.

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Most popular questions from this chapter

During a chemical reaction, NO(g) gets reduced and no nitrogen- containing compound is oxidized. Which of the following is a possible product of this reaction? (A) \(\mathrm{NO}_{2}(g)\) (B) \(\mathrm{N}_{2}(g)\) (C) \(\mathrm{NO}_{3}^{-}(a q)\) (D) \(\mathrm{NO}_{2}^{-}(a q)\)

$$\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightarrow 2 \mathrm{HI}(g)$$ When the reaction given above takes place in a sealed isothermal container, the rate law is $$\text { Rate }=k\left[\mathrm{H}_{2}\right]\left[\mathrm{I}_{2}\right]$$ If a mole of \(\mathrm{H}_{2}\) gas is added to the reaction chamber and the temperature remains constant, which of the following will be true? (A) The rate of reaction and the rate constant will increase. (B) The rate of reaction and the rate constant will not change. (C) The rate of reaction will increase and the rate constant will decrease. (D) The rate of reaction will increase and the rate constant will not change.

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