For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column.SystemChangeSA few moles of carbon dioxide (CO2) gas.The carbon dioxide is heated from 9.0 °C to 36.0 °C and also expands from a volume of 6.0 L to a volume of 14.0 L. <S0 =S0 >S0 not enough informationA few moles of helium (He) gas.The helium expands from a volume of 9.0 L to a volume of 15.0 L while the temperature is held constant at 20.0 °C. <S0 =S0 >S0 not enough informationA few grams of liquid ammonia (NH3).The ammonia is heated from -1.0 °C to 2.0 °C. <S0 =S0 >S0 not enough information

The entropy of a system increases due to any of the following reasons: 1. Increase in molecular weight and complexity of the molecule. 2. Increase in temperature 3. Decrease in pressure and increase in volume. 4. Change in phase from solid to liquid to gas, etc.#1: System: A few moles of carbon dioxide (CO2) gas. When we heat gas molecules, their energy increases. Hence they travel with more speed and collide with each other more frequently. Hence entropy increases when we increase temperature. Hence entropy increases. (Answer) #2: System: A few moles of Helium gas (He): When the helium gas expands from a volume of 9.0 L to a volume of 15.0 L, there are more space and ways for the molecules to distribute and expand energy. Hence entropy increases. (Answer) #3: System: A few grams of liquid ammonia (NH3): When we increase the temperature of molecules, their energy increases. Hence they travel with more speed and collide with each other more frequently. Hence entropy increases when we increase temperature. Hence entropy increases. (Answer)

Answered: For each system listed in the first…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy

of the system, decrease

, or leave

unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column.

System	Change	S
A few moles of carbon dioxide (CO₂) gas.	The carbon dioxide is heated from 9.0 °C to 36.0 °C and also expands from a volume of 6.0 L to a volume of 14.0 L.		<S0
	=S0
	>S0
	not enough information
A few moles of helium (He) gas.	The helium expands from a volume of 9.0 L to a volume of 15.0 L while the temperature is held constant at 20.0 °C.		<S0
	=S0
	>S0
	not enough information
A few grams of liquid ammonia (NH₃).	The ammonia is heated from -1.0 °C to 2.0 °C.		<S0
	=S0
	>S0
	not enough information

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