Question

Three moles of an ideal gas at 1 atm and 20°C are heated at constant pressure until the

final pressure at 80°C. for the gas Cv = 7.50 + 3.2 x 10-3

cal/ mole/ degree. Calculate W,

ΔE. ΔH and q.​

Answer 1

Answer:

80° 90°20°40°56°70°34°

Answer 2

Work done for the expansion of gas will be 1496.5 joule.

Explanation:

• Given that  Tintial(Ti)=20°C=293K    
• P=1 atm at constant pressure
• number of moles of an ideal gas =3 moles
• Tfinal(Tf)=80°C=353K

$Vi=\frac{nRTi}{p}$

$Vf=\frac{nRTf}{p}$

Work done w =$- PV$

$= -P(Vi-Vf)$

=$\frac{nR}{P}$×$(Tf-Ti)-1$----------1

Putting the value in equation 1

w= -3×8.314×(353-293)

w=1496.5

Work done for the expansion of gas will be 1496.5 joule.

$Cv = 7.50 + 3.2 x 10-3 cal/ mole/ degree$