Find the change in entropy when 2 g of nitrogen is cooled from 40

The change in entropy when cooling 2 grams of nitrogen from 400 K to 300 K can be found for two cases: at constant volume and at constant pressure.

At constant volume, the change in entropy can be found using the formula ΔS = C_v * ln(T2/T1), where ΔS is the change in entropy, C_v is the molar specific heat at constant volume, T1 and T2 are the initial and final temperatures, respectively. Substituting the values, we get:

ΔS = 2 * 20.8 * ln(300/400) = -8.97 J/K

At constant pressure, the change in entropy can be found using the formula ΔS = C_p * ln(T2/T1), where ΔS is the change in entropy, C_p is the molar specific heat at constant pressure, T1 and T2 are the initial and final temperatures, respectively. Substituting the values, we get:

ΔS = 2 * 29.1 * ln(300/400) = -12.60 J/K

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Find the change in entropy when 2 g of nitrogen is cooled from 400 K to 300 K

This digital product is a textbook on thermodynamics and allows you to calculate the change in entropy when 2 grams of nitrogen is cooled from 400 K to 300 K in two cases: at constant volume and at constant pressure.

• Calculates the entropy change when nitrogen is cooled
• Allows you to choose one of two cases: at constant volume or at constant pressure
• Convenient interface for entering start and end temperatures
• Fast and accurate calculation

Price: 200 rubles

Product description:

Our digital product is a thermodynamics textbook that allows you to calculate the change in entropy when cooling 2 grams of nitrogen from 400 K to 300 K in two cases: at constant volume and at constant pressure. Using a user-friendly interface, you can quickly and accurately enter the start and end temperatures and get the result. Our product has a number of advantages, including accuracy of calculations, user-friendly interface and the ability to choose one of two cases. Buy this study guide today for only 200 rubles and improve your knowledge in the field of thermodynamics!

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To solve this problem, you need to use the formula for entropy change ΔS = Cp * ln(T2/T1), where Cp is the isochoric heat capacity of the gas, T1 and T2 are the initial and final temperatures, respectively.

At constant volume Cp = (5/2)R, where R is the universal gas constant. At constant pressure Cp = (7/2)R.

It should also be taken into account that the change in entropy depends only on the initial and final temperatures, and not on the trajectory along which the process occurs.

Based on the problem conditions, initial temperature T1 = 400 K, final temperature T2 = 300 K, gas mass m = 2 g.

At constant volume: Cp = (5/2)R ΔS = Cp * ln(T2/T1) = (5/2)R * ln(300/400) ≈ -0.45R

At constant pressure: Cp = (7/2)R ΔS = Cp * ln(T2/T1) = (7/2)R * ln(300/400) ≈ -0.63R

Answer: When 2 g of nitrogen is cooled from 400 K to 300 K, the change in entropy is approximately -0.45R at constant volume, and approximately -0.63R at constant pressure.

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