Notifications
Clear all
0
06/10/2020 10:43 am
Topic starter
One mole of an ideal gas for which Cv = (3/2)R is heated reversibly at a constant pressure of 1 atm from 25°C to 100°C. The ΔH is :
(a) 3.775 cal
(b) 37.256 cal
(c) 372.56 cal
(d) 3725.6 cal
1 Answer
0
06/10/2020 10:46 am
(c) 372.56 cal
Explanation:
ΔH = ΔE + PΔV
[PV = RT; PΔV = RΔT, ΔE = ΔCv x (T2 - T1)]
= 3/2R x 75 + R x 75 = 75 x 5/2
= 372.56 cal