Question

For each system listed in the first column of the table below, decide whether the change described in the second column will increase the entropy S of the system, decrease, or leave S unchanged. If you don’t have enough information to deiced, check the “not enough information” button in the last column

System	Change	ϫS
A few moles of carbon CO2 gas	The carbon dioxide is cooled from -2 C to -9 Cwhile the volume is held constant at 10 L	ϫS < 0 ϫS = 0 ϫS > 0 not enough information
A few grams of liquid NH	The ammonia evaporates at a constant temperature of -3.0 C	ϫS < 0 ϫS = 0 ϫS > 0 not enough information
A few moles of CO2 gas	The carbon dioxide is heated from -1.0 C to 69 C and is also compressed from a volume of 9 L to a volume of 4 L	ϫS < 0 ϫS = 0 ϫS > 0 not enough information

Answer 1

Entropy is the measure of disorderness of system.

Entropy os gas > liquid > solid

Increase in temperature increases the entropy

Increase in volume increases the entropy

increase in pressure decreases the entropy

Now,

1. Since temperature of CO2 is decreased rom - 2 to - 9, the randomness of the system decreases and hence the entropy. So, delta S < 0

2. Since ammonia is geeting evaporates, its randomness will increase and hence the entropy. SO, deltaS > 0

3. Increase in temperature increases the entropy but decrease in volume decreases the entropy. Hence change in entropy depends on the net effect of temperature and volume.

SO, deltaS > 0