Complete combustion of hydrocarbons or compounds with C, H, and O as the only elements give CO₂ and H₂O as the only products. If carried out under standard conditions, the CO₂ is a gas and the H₂O is a liquid. Given these standard enthalpies of combustion:C₂H₄(g)= −1411.08 kJ mol⁻¹, C₆H₁₂(l)= −3919.86 kJ mol⁻¹, H₂(g)= −285.90 kJ mol⁻¹,C(s)= −393.50 kJ mol⁻¹, calculate ΔH°_reaction for the process: 3 C₂H₄(g)→ C₆H₁₂(l).Hint: Remember it is always products minus reactants when performing enthalpy calculations.

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The Answer of Complete combustion of hydrocarbons or compounds with C, H, and O as the only elements give CO₂ and H₂O as the only products. If carried out under standard conditions, the CO₂ is a gas and the H₂O is a liquid. Given these standard enthalpies of combustion:C₂H₄(g)= −1411.08 kJ mol⁻¹, C₆H₁₂(l)= −3919.86 kJ mol⁻¹, H₂(g)= −285.90 kJ mol⁻¹,C(s)= −393.50 kJ mol⁻¹, calculate ΔH°_reaction for the process: 3 C₂H₄(g)→ C₆H₁₂(l).Hint: Remember it is always products minus reactants when performing enthalpy calculations.

Complete Combustion of Hydrocarbons or Compounds with C, H, and O