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Chapter 12: Problem 28

Adding sidewalk deicer (calcium chloride) to water causes the temperature of the water to increase. If solid \(\mathrm{CaCl}_{2}\) is the system, what are the signs of \(\Delta S_{\mathrm{sys}}\) and \(\Delta S_{\mathrm{surr}} ?\)

Short Answer

Expert verified
Answer: When calcium chloride is added to water, the entropy change for both the system (solid calcium chloride) and the surroundings (water) is positive. This is due to the increased disorder in the system from dissolving the solid and the increased temperature of the water, causing increased disorder in the surroundings.

Step by step solution

01

1. Determine the entropy change of the system

Since the system is solid calcium chloride, dissolving in water, the system's entropy will increase. This is because the solid calcium chloride particles are scattered through the water, leading to an increase in disorder. Therefore, 螖S_sys is positive. 螖S_sys > 0
02

2. Determine the entropy change of the surroundings

When the solid calcium chloride dissolves in water, it causes the temperature of the water to increase. An increase in temperature leads to an increase in the entropy of the surroundings. This is because the water molecules will move more rapidly as the temperature increases, causing more disorder in the surroundings. So, 螖S_surr is positive. 螖S_surr > 0
03

3. Summarize the signs of 螖S_sys and 螖S_surr

In conclusion, the entropy change of both the system (solid calcium chloride) and the surroundings (water) is positive when CaCl鈧� is added to water.

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Why is it important that at least some of the spontaneous steps in glycolysis convert ADP to ATP?

What are the signs of \(\Delta S, \Delta H,\) and \(\Delta G\) for the sublimation of dry ice (solid \(\mathrm{CO}_{2}\) ) at \(25^{\circ} \mathrm{C} ?\)

Which of the following combinations of entropy changes for a process are mathematically possible? a. \(\Delta S_{\text {sys }}>0, \Delta S_{\text {surr }}>0, \Delta S_{\text {univ }}>0\) b. \(\Delta S_{\text {sys }}>0, \Delta S_{\text {surr }}<0, \Delta S_{\text {univ }}>0\) c. \(\Delta S_{\text {sys }}>0, \Delta S_{\text {surr }}>0, \Delta S_{\text {univ }}<0\)

Which component in each of the following pairs has the greater entropy? a. 1 mole of \(\mathrm{S}_{2}(g)\) or 1 mole of \(\mathrm{S}_{8}(g)\) b. 1 mole of \(S_{2}(g)\) or 1 mole of \(S_{8}(s)\) c. 1 mole of \(\mathrm{O}_{2}(g)\) or 1 mole of \(\mathrm{O}_{3}(g)\)

In which direction does a reaction proceed when (a) \(\Delta G_{\text {rxn }}<0 ;\) (b) \(\Delta G_{\text {rxn }}=0 ;\) (c) \(\Delta G_{\text {ren }}>0 ?\)
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