The balanced combustion reaction for C6H6 is 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ 2 ⁢ C 6 ⁢ H 6 ⁡ ( l ) + 15 ⁢ O 2 ⁡ ( g ) ⟶ 12 ⁢ CO 2 ⁢ ( g ) + 6 ⁢ H 2 O ( l ) + 6542 kJ

Question

The balanced combustion reaction for C6H6 is2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ

If 6.600 g C6H6 is burned and the heat produced from the burning is added to 5691 g of water at 21 ∘C, what is the final temperature of the water?

Answer 1

Very little change in temperature, as we only have a fraction of a mole of Benzene to burn. I also didn't realize that the question gives you the energy produced from the reaction. If you take that number (6542 kJ) and divide by 2 (because the balanced equation requires 2 moles of Benzene), you get roughly the same H value I used.