Question
For the complete combustion of ethanol, C2H5OH (l) + 3O2 (g) → 2CO2 (g) + 3H2O (l), the amount of heat produced as measured in a bomb calorimeter, is 1364.47 kJ mol-1 at 25oC. Assuming ideality the enthalpy of combustion, ∆CH, for the reaction will be (R = 8.314 JK-1 mol-1)
-
-1366.95 kJ mol-1
-
-1361.95 kJ mol-1
-
-1460.50 kJ mol-1
-
-1350.50 kJ mol-1
Solution
A.
-1366.95 kJ mol-1
C2H5OH (l) + 3O2 (g) → 2CO2 (g) + 3H2O (l),∆U = - 1364.47 kJ/mol
∆H = ∆U +∆ngRT
∆ng = -1
∆H = - 1364.47 +
[Here, value of R in unit of J must be converted into kJ]
= - 1364.47-2.4776
= -1366.94 kJ/mol
∆ng = -1
∆H = - 1364.47 +
[Here, value of R in unit of J must be converted into kJ]
= - 1364.47-2.4776
= -1366.94 kJ/mol
