A certain gas is expanded from (1 L, 10 atm) to (4 L, 5 atm) against a constant external pressure of 1 atm. If the initial temperature of the gas is 300 K and the heat capacity for the process is 50J/C0, the enthalpy change during the process is :
A
15 kJ
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
15.7 kJ
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C
14.3 kJ
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
14.7 kJ
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution
The correct option is B 15.7 kJ The amount of gas expanded using the ideal gas equation: P1V1=nRT1 10×1=n×0.0821×300 n = 0.4 mole Final temperature obtained: P2V2=nRT2 5×4=0.4×0.0821×T2 T2 = 600 K Work done during expansion = −Pext(V2−V1) = -1(4-1) atm L = 300 J and heat involved = Q=CpdT = 50×(600−300) = 15000 J Using equation δU=δQ+δW = 15000-300 = 14700 J and δH=δU+δ(PV) = 14700 + (4×5−10×1)×100 J =15700J = 15.7 kJ