Answer:
929.4 kJ of heat is released.
Explanation:
The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0 °C.
The data explains that 1 mol of H₂S uses 18.7 kJ of energy in vaporization.
By the Ideal Gas Law, we can know, how many moles do we have, of gas.
P. V = n . R . T
87 atm . 10L = n . 0.0821 L.atm/K.mol . 213 K
(87 atm . 10L) / (0.0821 K.mol/L.atm . 213 K) = 49.7 moles
1 mol ____ 18.7 kJ
49.7 moles _____ (49.7 . 18.7) = 929.4 kJ
