Calculate the work (w) and ΔEo, in kJ, at 298 K and 1
atm pressure, for the combustion of one mole of
C4H10 (g). First write and balance the
equation. The products will be CO2 (g) and
H2O (g).
The value of ΔHo for this reaction is -2658.3
kJ/mol.
The value for w in kJ =
The value for ΔEo ( in kJ) =
C4H10 (g) + 6.5 O2(g) ---> 4
CO2(g) + 5 H2O(g)
Dnrxn = no of mole of Products - no of mole of Reactants
= (4+5) - (1+6.5)
= 1.5
work done (w) = -DnRT
= -1.5*8.314*298
= -3.716 kj
DH = DU + DnRT
(-2658.3) = x - 3.716
DU = -2654.6 kj
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