posted by Kat on .
Use standard heats of formation in Appendix L to calculate standard enthalpy changes for the following reactions.
1.45 x 10-2 mol of carbon is oxidized to CO2(g)
Please help me!
Look up the heat of formation for CO2 in the table provided to you. My table has something like 393.5 kJ/mol. That reaction is for
C + O2 ==> CO2
delta H reaction is (n*deltaHf products) - (n*deltaHf reactants) =
(n*deltaHf CO2) - [(n*deltaHf C) + (n*deltaHf O2)]
delta Hrxn = -393.5 -(+0) = -393.5 kJ/mol.
You have 1.45E-2 mol instead of 1 mole; therefore, delta H rxn = -393.5 kJ/mol x 1.45E-2 mol = ?? kJ.
Thank you! but does n in (n*deltaHf products) - (n*deltaHf reactants) mean amount? What amount is it talkinging about?