College Physics
College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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Question

As a 3.00-mol sample of a monatomic ideal gas expands adiabatically, the work done on it is −2.50  103 J. The initial temperature and pressure of the gas are 400 K and 2.60 atm. Calculate the following.

(a) the final temperature
 K

(b) the final pressure
 atm
Expert Solution
Check Mark
Step 1

Given:

         Number of moles(n) = 3

        Initial temperature(Ti) = 400 K

       Initial pressure(Pi) = 2.6 atm

      Work done(w) = - 2.5×103 J

(a).

work done in adiabatic process

⇒ w = n cvR(Tf - Ti)

Here, cv for monoatomic is 32; and R = 8.314 J/mol.k

⇒ - 2.5×103 = 3×32×8.314(Tf - 400)

⇒ Tf =- 5×1039×8.314 + 400

⇒ Tf = 333.18 K

Therefore the final temperature is 333.18 K

 

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