Calculate the heat of combustion of ethylene (gas) to form CO2 (gas) a

1.	Calculate the heat of combustion of ethylene (gas) to form CO2 (gas) and H2O (gas) at 298 K and 1 atmospheric pressure. The heats of formation of CO2, H2O and C2H4 are -393.7 - 241.8 + 52.3 kJ per mole respectively.
Answer» C₂H₄ (g) + 3O₂ (g) → 2CO₂ (g) + 2H₂O (g) ΔH_f(CO₂) = -393.7 kJ ΔH_f(H₂O) = -241.8 kJ ΔH_f(C₂H₄) = +52.3 kJ ΔH_Reaction = (Sum of ΔH°_f values of products) - (Sum of ΔH°_f value of reactants) = [2 x ΔH°_f(CO₂) + 2 x ΔH°_f(H₂O) - [ΔH°_f(C₂H₄) + 3 x ΔH°_f(O₂)]] = 2 x (-393.7) + 2 x )-241.8) - [523.0 + 0] [∵ ΔH°_f for elementary substance = 0] = [-787.4 - 483.6] - 53.3 = -1323.3 kJ

Calculate the heat of combustion of ethylene (gas) to form CO2 (gas) and H2O (gas) at 298 K and 1 atmospheric pressure. The heats of formation of CO2, H2O and C2H4 are -393.7 - 241.8 + 52.3 kJ per mole respectively.

Answer»

C₂H₄ (g) + 3O₂ (g) → 2CO₂ (g) + 2H₂O (g)

ΔH_f(CO₂) = -393.7 kJ

ΔH_f(H₂O) = -241.8 kJ

ΔH_f(C₂H₄) = +52.3 kJ

ΔH_Reaction = (Sum of ΔH°_f values of products) - (Sum of ΔH°_f value of reactants)

= [2 x ΔH°_f(CO₂) + 2 x ΔH°_f(H₂O) - [ΔH°_f(C₂H₄) + 3 x ΔH°_f(O₂)]]

= 2 x (-393.7) + 2 x )-241.8) - [523.0 + 0]

[∵ ΔH°_f for elementary substance = 0]

= [-787.4 - 483.6] - 53.3

= -1323.3 kJ

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Calculate the heat of combustion of ethylene (gas) to form CO2 (gas) and H2O (gas) at 298 K and 1 atmospheric pressure. The heats of formation of CO2, H2O and C2H4 are -393.7 - 241.8 + 52.3 kJ per mole respectively.

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