2C4H10 + 13O2  -> 8 CO2 + 10 H2O   Heat= -5314kJ, heat of combustion per gram?

The enthalpy (or heat) of combustion of acetone, (CH3)2CO, is - 1657.8 kJ. The reaction is (CH3)2CO (1) +4 0₂ (g) →3 CO₂(g) + 3 H₂O (g). Given the values of AH-393.5 kJ/mol for CO₂ (g) and AH-241.8 kJ/mol for H₂O(g), the calculated value of AH; for acetone O equals - 3563.7 kJ/mol O equals - 1022.5 kJ/mol O equals-248.1 kJ/mol O equals 1202.7 kJ/mol

18. From the following data, AH = -393.5 kJ/mol C(graphite) + O₂(g) → CO₂(g) 1 H₂ (g) + O₂(g) → H₂O(l) AH = -285.8 kJ/mol 2C₂H6 (g) +70₂(g) → 6H₂O(l) + 4CO₂(g) AH = -3119.06 kJ/mol calculate the enthalpy change for the reaction: 2C (graphite) (1) + 3H₂(g) → 2C₂H6 (g)

For the reaction below (which will be labeled reaction A), the reaction enthalpy is unknown:                                                   2 B    + 3 H2    B2H6    HA  = ? Use the following thermochemical data to calculate the reaction enthalpy ΔHA: Reaction 1:       4 B + 3 O2 → 2 B2O3                               ΔH1 = –2509 kJ Reaction 2:       2 H2 + O2 → 2 H2O                          ΔH2 = –572 kJ Reaction 3:       B2H6 + 3 O2 → B2O3 + 3 H2O   ΔH3 = –2,159 kJ Calculate the enthalpy of reaction A (in kJ) and enter the numerical value in the answer box. Do not write units in the answer box. Clearly show on a paper how each reaction can be combined to equal reaction A  (multiply or reverse  each of the above reactions).complete work must be uploaded