Three moles of an ideal monatomic gas expands at a constant pressure of 2.50 atm; the volume of the gas changes from 3.20 X 10-2 m3 to 4.50 X 10-2 m3. Calculate (a) the initial and final temperatures of the gas; (b) the amount of work the gas does in expanding; (c) the amount of heat added to the gas; (d) the change in internal energy of the gas.

Solution 24E Problem (a) Step 1: Pressure P = 2.50 atm or 2.53 x 10 Pa (constant) Initial Volume V = 3.20 x 10 2 m 3 1 2 3 Final VolumeV 2 = 4.50 x 10 m No of moles n = 3 moles Gas constant R = 8.314 J/mol.K Step 2: Initial temperature T 1 From Ideal gas equation PV = nRT T = PV 1 1 nR 2.5* 10*3.2* 10 T 1 = * 8.314 T 1 = 326 K Step 3: Final temperature T 2 PV T 2 = nR2 T = 2.5* 10*4.* 10 2 3*8.314 T 2 = 456.5K Problem (b) Step 1: Amount of work done in expanding W = P.dV W = P.(V 2...