Benzaldehyde and Benzoic AcidHard
Question
The heat of combustion of benzoic acid at constant volume is - 321.3 kJ at 27oC. The heat of combustion at constant pressure is. (R = 8.314 JK-1 mol-1). Reaction is :
C6H5COOH(l) +15/2 O2(g) → 7CO2(g) + 3H2O(l)
C6H5COOH(l) +15/2 O2(g) → 7CO2(g) + 3H2O(l)
Options
A.-321.3 kJ
B.-322.54 kJ
C.+322.54 kJ
D.+321.3 kJ
Solution
ᐃE = qv = - 321.3 kJ/mol
ᐃH = qp = ᐃE + (ᐃng)RT
C6H5COOH(l) +
O2(g) → 7CO2 (g) + 3H2O(l)
ᐃng = 7 -
ᐃH = -321.3 +
(8.314) (300) × 10-3
= - 322.54 kJ
ᐃH = qp = ᐃE + (ᐃng)RT
C6H5COOH(l) +
O2(g) → 7CO2 (g) + 3H2O(l)ᐃng = 7 -
ᐃH = -321.3 +
(8.314) (300) × 10-3= - 322.54 kJ
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