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

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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