Balance the following reaction and use the equation to calculate the ΔHrxn. C3H8 (g) + O2 (g) → CO2 (g) + H2O (g) Round your answer to the nearest whole number. ΔHrxn=kJ/mole

The reaction corresponds to the combustion of propane (C3H8). The balanced reaction is:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)

The reaction enthalpy is given as:

ΔHrxn = ∑nΔH°f (products) - ∑ nΔH°f (reactants)

= [3ΔH°f (CO2 (g)) + 4ΔH°f (H2O (g) ] - [1ΔH°f (C3H8 (g)) + 5ΔH°f (O2 (g) ]

= [3 (-393.5) + 4 (-241.8) ] - [-103.9 + 5 (0) ] = - 2043.8 kJ

The enthalpy for the combustion of propane is - 2044 kJ