ThermodynamicsHard
Question
Consider the reaction: N2 + 3H2 → 2NH3 carried out at constant temperature and pressure. If ᐃH and ᐃU are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?
Options
A.ᐃH = 0
B.ᐃH = ᐃU
C.ᐃH < ᐃU
D.ᐃH > ᐃU
Solution
ᐃH = ᐃU + ᐃnRT
ᐃn = - 2
ᐃH = ᐃU - 2RT
ᐃH < ᐃU
ᐃn = - 2
ᐃH = ᐃU - 2RT
ᐃH < ᐃU
Create a free account to view solution
View Solution FreeMore Thermodynamics Questions
On the basis of the following thermochemical data : (áƒGfoH+(aq) = 0) H2O(l) → H+ (aq) + OH-(aq); áƒH = 57.32 kj ...In any natural process :-...N2 + 3H2 ⇋ 2NH3 Which is correct statement if N2 is added at equilibrium condition?...A monoatomic gas expands isobarically. The percentage of heat supplied that increases the thermal energy and that involv...Three samples A, B and C of the same ideal gas ($\gamma$ = 1.5) have equal volumes and temperatures. The volume of each ...