posted by Alexa
The homework question is :
Calculate the Delta H for the following reaction:
C6H6 + O2 -> C + H2O(l)
State whether the reaction is exothermic or endothermic.
I'm not sure where to go with this but so far I balanced out the formula to this
C6H6 + (3/2)O2 -> 6C2 + 3H2O
I found online that the standard enthalpy of formation of C6H6 is 48.95 kJ/mol but where do I go from there?
Is that the equation given for the reaction? USUALLY the products are CO2 and H2O. At any rate, here is what you do.
Yes, balance the equation. Then
dHrxn = (n*dHf procuts) - (n*dHf reactants)
Look up the dHf in your text or notes. Lots of places on the net also. By the way, for C I would not write it as C2 AND you will need to know if it is graphite or not.
dHrxn is - it is exothermic; if + endothermic.
I think it is an error. Usually we have to get CO2 instead of C as it is a combustion reaction and in theory it is an exothermic reaction