# Energy balance question

This was a question from one of my tutes earlier in the semester, and now that I'm revising for an exam I can't seem to remember how to do it.
If anyone can help that would be great!

Sulfuric acid is a major bulk chemical used in a wide variety of industries. After sulfur is
oxidized to SO2, the SO2 is further oxidized in the converters (reactors) to SO3
SO2 (g) + ½ O2 (g) + SO3 (g)
and the SO3 is absorbed in dilute H2SO4 to form concentrated H2SO4
In the first converter the entering gases at 400K and 1 atm are composed of 9.0% SO2, 9.5%
O2, and 81.5% N2. Only 75% of the entering SO2 reacts on going through the first converter.
If the maximum temperature of the gas before going to the next converter (where the reaction
is completed) can be 700K, how much heat must be removed from the gas before it goes to
the second converter per kg mol of gases entering the process?

Data:
Heat capacities of gases in J/gmol oC. Temperature in oC.
N2: 29.00 + 0.2199 x 10-2 T + 0.5732 x 10-5 T2
O2: 29.10 + 1.158 x 10-2 T - 0.6076 x 10-5 T2
SO2: 38.91 + 3.904 x 10-2 T – 3.104 x 10-5 T2
SO3: 48.50 + 9.188 x 10-2 T – 8.540 x 10-5 T2
Standard heat of formation (kJ/gmol):
SO2: -296.9 kJ/gmol
SO3: -395.18 kJ/gmol

thanks a lot :)