For each system listed in the first column of the table below, decide (if possib

Question

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 System Change The carbon dioxide is cooled from 81.0 °C to -11.0 °c and is also expanded from a volume of 9.0 L to a volume of 15.O L A few moles of carbon dioxide (CO2) gas. > 0 not enough information The water is heated from -20.0 °C to 71.0 °C. A few grams of liquid water (H20 not enough information The helium expands from a volume of 4.0 L to a volume of 5.0 L while the temperature is held constant at 45.0 °C. ?S = 0 ? S > 0 not enough A few moles of helium (He) gas. information

Explanation / Answer

Entropy change during process

System : few moles of CO2 gas

Change : cooled and exapanded

Entropy change : dS > 0

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System : few grams of liquid water

Change : heated

Entropy change : dS > 0

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System : few moles of He gas

Change : exapanded at constant T

Entropy change : dS > 0

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