ThermochemistryHard
Question
The heat of reaction for : C10H8(s) + 12O2(g) → 10CO2(g) + 4H2O(l) at constant volume is 1228.2 kcal at 25oC. The heat of reaction at contant pressure and same temperature is :
Options
A.-1228.2 kcal
B.-1229.3 kcal
C.-1232.9 kcal
D.1242.6 kcal
Solution
ᐃE = - 1228.2Kcal = 1228.2 × 103cal
ᐃH = ᐃE + ᐃnRT
1228.2 × 103 = (-2)(2)(298)
= - 1229392 cal
= - 1229.392 kcal
ᐃH = ᐃE + ᐃnRT
1228.2 × 103 = (-2)(2)(298)
= - 1229392 cal
= - 1229.392 kcal
Create a free account to view solution
View Solution FreeMore Thermochemistry Questions
Enthalpy change for the reaction,4H(g) → 2H2 (g) is - 869.6 kJ The dissociation energy of H - H bond is...For the given reactionsSiO2 + 4HF → SiF4 + 2H2O, ᐃH = -10.17 kcalSiO2 + 4HCl → SiCl4 + 2H2O, ᐃH ...For the equilibrium H2O(l) ⇋ H2O(g) at 1atm and 298 K :...Using the data provided, calculate the multiple bond energy (kJ mol-1) of a C ≡ C bond in C2H2. That energy is (take t...When 1.0 g of oxalic acid (H2C2O4) is burned in a bomb calorimeter whose heat capacity is 8.75 kJ/K, the temperature inc...