This question has three paarts:
1. Determine the mass of water formed when 14.5L NH3 (at 298K and 1.5 atm) is reacted with 19.3 L of O2 (at 321K and 1.2 atm)
4NH3+O2-->4NO+6H2O
I got the answer of 19 g H2O
2.What are the partial pressures for all gases that remain at the end, if the reaction took place in a sealed 50.0L tank and the final temperature is 345K? (some reactants will be left over)
I didn't find 10 g H2O; something more like 23 or so. Post your work and someone will find the error. I'm sure you determined the limiting reagent.
For part 2, using the limiting reagent and the moles of each material formed, use PV = nRT to calculate partial pressure. For the non-limiting reagent, calculate the amount un-reacted, convert to moles (unless you used moles for this part), and use PV = nRT to calculate pressure.