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Thermodynamics : Heats of Formation

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For the reaction CH4 (g) + N2 (g) + 164 kJ 6 HCN(g) + NH3 (g) at 25degrees C and 1 atm of pressure
ÄGo = 159 kJ. Calculate ÄSo at 25degrees C.

ÄHfo for CH4 (g) = -74.77 kJ/mol and ÄHfo for
NH3 (g) = -46.09 kJ/mol. What is ÄHfo for HCN(g) ?

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For the reaction CH4 (g) + N2 (g) + 164 kJ 6 HCN(g) + NH3 (g) at 25degrees C and 1 atm of pressure
ÄGo = 159 kJ. Calculate ÄSo at 25degrees C.

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Solution Summary

This solution explains how to calculate entropy based on Gibbs free energy and enthalpy of formation. This solution also explains how to calculate the heat of formation of a compound using the heat of reaction.

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Thermodynamics and Enthalpy of Formation

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).

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