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1.1 mole of O₂ (g) and 2.2 moles of N₂ (g) are spontaneously mixed in a cylinder (volume = 30.0 L) with a movable piston. Assume both gases are ideal. (a) Explain why the mixing of O₂ and N₂ gases is spontaneous in term of chemical potential. (b) Calculate the final pressure (in N m2) of mixture when (i) the mixing occurs isothermally at 298 K; (ii) the initial temperatures of O₂ (g) and N₂ (g) are 306 K and 367 K, respectively, and after mixing, the temperature is equilibrated. State any assumption(s) in your calculations. (c) Now, the mixture in (b)(ii) is expanded isothermally and the external pressure is suddenly decreased to a final pressure of 890 Torr, determine whether the process is reversible or

1.1 mole of O₂ (g) and 2.2 moles of N₂ (g) are spontaneously mixed in a cylinder (volume = 30.0 L) with a movable piston. Assume both gases are ideal. (a) Explain why the mixing of O₂ and N₂ gases is spontaneous in term of chemical potential. (b) Calculate the final pressure (in N m2) of mixture when (i) the mixing occurs isothermally at 298 K; (ii) the initial temperatures of O₂ (g) and N₂ (g) are 306 K and 367 K, respectively, and after mixing, the temperature is equilibrated. State any assumption(s) in your calculations. (c) Now, the mixture in (b)(ii) is expanded isothermally and the external pressure is suddenly decreased to a final pressure of 890 Torr, determine whether the process is reversible or

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.103QE: A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it...
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1.1 mole of O₂ (g) and 2.2 moles of N₂ (g) are spontaneously mixed in a cylinder (volume = 30.0 L) with a movable piston. Assume both gases are ideal. (a) Explain why the mixing of O₂ and N₂ gases is spontaneous in term of chemical potential. (b) Calculate the final pressure (in N m2) of mixture when (i) the mixing occurs isothermally at 298 K; (ii) the initial temperatures of O₂ (g) and N₂ (g) are 306 K and 367 K, respectively, and after mixing, the temperature is equilibrated. State any assumption(s) in your calculations. (c) ) Now, the mixture in (b)(ii) is expanded isothermally and the external pressure is suddenly decreased to a final pressure of 890 Torr, determine whether the process is reversible or not.
Transcribed Image Text:1.1 mole of O₂ (g) and 2.2 moles of N₂ (g) are spontaneously mixed in a cylinder (volume = 30.0 L) with a movable piston. Assume both gases are ideal. (a) Explain why the mixing of O₂ and N₂ gases is spontaneous in term of chemical potential. (b) Calculate the final pressure (in N m2) of mixture when (i) the mixing occurs isothermally at 298 K; (ii) the initial temperatures of O₂ (g) and N₂ (g) are 306 K and 367 K, respectively, and after mixing, the temperature is equilibrated. State any assumption(s) in your calculations. (c) ) Now, the mixture in (b)(ii) is expanded isothermally and the external pressure is suddenly decreased to a final pressure of 890 Torr, determine whether the process is reversible or not.
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