[Boosted55]

I'm currently having troubles trying to calculate the change in enthalpy and partial pressure. Any help would be apperciated!! Here's the problems:

What is the change in enthalpy (in kJ) under standard conditions when 9.8 g of benzene is combusted?

Here is the answer I calculated, but was incorrect..
2C6H6 (l) + 15O2 (g) ---> 12CO2 (g) + 6H2O (l)

(12)-393.5 + -2361 - (2)-124.7 = -1781.2 kJ
9.8 g C6H6 x (1 mol/ 78.1 g) = .125 mole x -1781.2 kJ = -222.65 kJ

Nitrogen and hydrogen react in the Haber process to form ammonia. All substances are in the gas phase. If 0.377 atm of nitrogen and 0.802 atm of hydrogen react, what is the partial pressure of ammonia (in mmHg) when this reaction goes 83.8 complete. The volume and temperature are constant.

N2 + 3H2 = 2NH3

Here, I wasnt sure where to start, other then writing and balancing the equation.

Thanks!!