I don't know what you next motive is but I suggest this for your next move. And note that I've corrected your equation for the typos.
C6H12 + 9O2 ==> 6CO2 + 6H2O
First determine what the limiting regent is.
mols cyclohexane = 32/84.2 = about 0.38
mols.
mols O2 from your work = 4.24
If 0.38 g cyclohexane reacts with an excess of O2, it will produce 0.38 x (6 mol CO2/1 mol C6H12) = about 2.28mol CO2.
If 4.24 mol O2 react with excess C6H12, CO2 produced is 4.24 x (6 mols CO2/9 mols O2) = 4.24 x 6/9 = about 2.83 mol CO2. Therefore, C6H12 is the limiting reagent and you have used all of it or 0.38 mols.
Then 1 mol produces 3690 kJ so you have
3690 kJ/mol x 0.38 mol = ? heat in kJ.
C6H12 = 9O2 --> 6CO2 = 6H2O + 3,690 kJ
*Personally Balanced*
What quantity of heat is produced if 32g of cyclohexane react with 95 L of oxygen at STP?
*My work so far is below*
95L*(1 mol O2/22.4L) = 4.2 mol O2
What would be the next motive?
2 answers
the answer we get it as 1402.2KJ
3 answers