I need help with Chemistry

Question

1. Methane (CH4) is a highly flammable gas that can combust according to the equation below: 

CH4 (g) + 2 O2 (g) → 2 H2O (g) + CO2 (g)

a.)Given the standard heats of formation (ΔHof) in the table below, calculate the ΔH of the combustion reaction.

1. 
   

Compound	∆Hf° (kJ/mol)
CO2 (g)	–393.5
H2O (g)	-241.8
H2O (l)	-285.8
CH4	-74.87

b.)Use the ΔHcombustion from part (a) and the bond enthalpies in the table below to determine the bond enthalpy per mole of O2

1. 
   

Bond Type	Average Bond Enthalpy (kJ/mol)
C - H	414
C - O	360
C = O	799
O - H	464
O = O	?

c.)Draw a reaction profile for the combustion of methane. Use a vertical arrow (↕️) to indicate ΔHcombustion that you calculated in (a)

Answer 1

Please let me know if that makes sense