(d) A quantity of n = 2.0 mol of an ideal gas with Cv,m = 20.8 J K¹ mol¹ is initially at p = 330 kPa and T = 310 K. It undergoes reversible adiabatic expansion until the pressure reaches 250 kPa. Calculate (i) the final volume, (ii) the final temperature and (iii) the work done in the process.

(d) A quantity of n = 2.0 mol of an ideal gas with Cv,m = 20.8 J K¹ mol¹ is initially at p = 330 kPa and T = 310 K. It undergoes reversible adiabatic expansion until the pressure reaches 250 kPa. Calculate (i) the final volume, (ii) the final temperature and (iii) the work done in the process.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter1: Gases And The Zeroth Law Of Thermodynamics

Section: Chapter Questions

Problem 1.65E: Determine an expression for V/T p, n in terms of and . Does the sign on the expression make sense...

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Question

(d) A quantity of n = 2.0 mol of an ideal gas with Cv,m = 20.8 J K¹ mol¹ is initially at
p = 330 kPa and T = 310 K. It undergoes reversible adiabatic expansion until the
pressure reaches 250 kPa. Calculate (i) the final volume, (ii) the final temperature
and (iii) the work done in the process.

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