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:C₂H₂(g)= −1299.65 kJ mol⁻¹, C₆H₆(l)= −3267.80 kJ mol⁻¹, H₂(g)= −285.90 kJ mol⁻¹,C(s)= −393.50 kJ mol⁻¹, calculate ΔH°_reaction for the process, 3 C₂H₂(g)→ C₆H₆(l).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:C₂H₂(g)= −1299.65 kJ mol⁻¹, C₆H₆(l)= −3267.80 kJ mol⁻¹, H₂(g)= −285.90 kJ mol⁻¹,C(s)= −393.50 kJ mol⁻¹, calculate ΔH°_reaction for the process, 3 C₂H₂(g)→ C₆H₆(l).Remember it is always products minus reactants when performing enthalpy calculations.

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