Use the thermochemical equations shown below to determine the enthalpy for the reaction: H2SO4(l)=>H2S(g) +

Use the thermochemical equations shown below to determine
the enthalpy for the reaction:

H2SO4(l)=>H2S(g) + 2O2(g)

SO3(g) + H2O(g)=>H2SO4(l) H=-251.1KJ

H2S(g) + 2O2(g)=>SO3(g) + H2O(l) H=-845.2KJ

H2O(l)=>H2O(g) H=134.8KJ


I put 961.5KJ but it's wrong, explain please

H2SO4(l) => SO3(g) + H2O(g) H=+251.1KJ

SO3(g) + H2O(l) => H2S(g) + 2O2(g)= H=+845.2KJ

H2O(g)=>H2O(l) H=-134.8KJ

I get 961.5 as well. Round if off to 962??? Also, it could be a data entry error in whatever you are using (like a computer-based system or a printing error in an answer in your textbook.) In any event, you did the problem did the problem correctly, I think, in my status as just some guy on the Internet, that ice cream is the right choice at this moment in your life.

More Hess' Law:

http://www.chemteam.info/Thermochem/Ther…