I need some help with this problem, see attached file for full problem description with proper symbols:
2. a) Use only the following data to determine delta H°f for NO2 (g):
- delta H°f for NO (g) is +90.4 kJ/mol
- delta H = -56.6 kJ/mol for the reaction: NO (g) + 1/2 O2 (g) ---> NO2 (g)
b) Find delta H for the reaction: 4 CO (g) + 2 NO2 (g) ----> 4 CO2 (g) + N2 (g)
using only your answer to (a) and the fact that
delta H = -283.0 kJ/mol for the reaction: CO (g) + 1/2 O2 (g)------> CO2 (g)
c) A 10.0-liter vessel contains 5.0 atm of CO and 3.0 atm of NO2 at 25°C. How
much heat (in Joules) will be liberated if this is allowed to react to completion
according to the reaction in part (b)?
d) With Appendix C from your text, calculate H for the combustion of C4H10 (l).
This solution gives step-by-step calculations to determine delta H for NO2, conversion of carbon monoxide to carbon dioxide and also how much heat is liberated if a reaction is allowed to react to completion. Full workings and explanations are provided.