The calculated enthalpy of formation of kerosene is 365.4 kJ and heat produced is 78650.3 kJ
For this, we need the normal enthalpy of formation given below
ΔH∘f(CO2)=−393.5kJ/molΔH∘f(H2O)\s=−241.8kJ/molΔH∘f(O2)=0kJ/mol
We shall now determine the enthalpy of kerosene formation:
H rxn = 24 mol H f (CO2) + 26 mol H f (H2O) + 2 mol H f (C12H26) + 37 mol H f (O2) + 1.50 104 kJ = 9444 kJ + 6286.8 kJ + 1500 kJ 2 mol H f (C12H26) = 730.8 kJ H f (C12H26) = 365.4 kJ
Kerosene has a density of 0.74 g/mL.
Kerosene volume (V) equals 0.63 gallons, or 0.63 x 3785.4, or 2384. 8 mL.
We shall now calculate the mass (m) of kerosene:
ρ=mVm\s=ρ×Vm\s=0.749g/mL×2384.mLm\s=1786.2g
We shall now discover the heat that 1786 generated.
Two grams of kerosene
Kerosene's molar mass is 170.33 g/mol.
The mass of two moles of kerosene is equal to 2*170.33*340.66g.
1.50104kJ of heat are generated by 340.66 g of kerosene.
1786 produced heat.
Kerosene 2 grams = 1.50 104 kJ 340.66 1786.2 g = 78650.3 kJ
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