Calculate the change in entropy for the system, the surroundings and the Universe if 2 moles of ethane are completely combusted at 298 K. Standard entropies of C2H5(g), O2(g), H2O(l) and CO2(g) are 229.6, 205.1, 69.9, 213.7 J mol-1 K-1 , respectively. Standard enthalpy changes of formation of C2H5(g), H2O(l) and CO2(g) are -83.8, -285.8 and -393.5 kJ mol-1 , respectively. I know that ΔS= Σproduct -Σreactants and that ΔS(uni)=ΔS(sys)+ΔS(surr)=0. But the question is worth 12.5 marks and I haven't even used the enthalpy values or moles. Are those enthalpy values there to throw me off or am I missing something? Any help is greatly appreciated and thanks in advance!