will fan and medal!!!
What is the ∆G for the following reaction under standard conditions (T = 298 K) for the formation of NH4NO3(s)?
2NH3(g) + 2O2(g) NH4NO3(s) + H2O(l)

Given:
NH4NO3(s): ∆Hf = -365.56 kJ ∆Sf = 151.08 J/K.
NH3(g): ∆Hf = -46.11 kJ ∆Sf = 192.45 J/K.
H2O(l): ∆Hf = -285.830 kJ ∆Sf = 69.91 J/K.
O2(g): ∆Hf = 0.00 kJ ∆Sf = 205 J/K.
a. 186.6 kJ
b. 6.9 kJ
c. -10.4 kJ
d. -126.3 kJ
e. -382 kJ

Question

will fan and medal!!!
What is the ∆G for the following reaction under standard conditions (T = 298 K) for the formation of NH4NO3(s)? 
2NH3(g) + 2O2(g)  NH4NO3(s) + H2O(l)

Given:
NH4NO3(s): ∆Hf = -365.56 kJ ∆Sf = 151.08 J/K. 
NH3(g): ∆Hf = -46.11 kJ ∆Sf = 192.45 J/K. 
H2O(l): ∆Hf = -285.830 kJ ∆Sf = 69.91 J/K. 
O2(g): ∆Hf = 0.00 kJ ∆Sf = 205 J/K.
a. 186.6 kJ
b. 6.9 kJ
c. -10.4 kJ
d. -126.3 kJ
e. -382 kJ

fmnsmythe · Answer

Please help!

amtran_bus · Answer

Delta G = Delta H - T Delta S

frostbite · Answer

You could help a little by saying that he needs to calculate the enthalpy and entropy OF THE REACTION in order to calculate the Gibbs free energy OF THE REACTION.

sweetburger · Answer

$$\Delta H=\sum_{}^{}\Delta  H_\left( products \right)-\sum_{}^{}\Delta  H_\left( reactants \right)$$
and
$$\Delta S =\sum_{}^{}\Delta  S_\left( products \right)-\sum_{}^{}\Delta  S_\left( reactants \right)$$

sweetburger · Answer

these equations will be pertinent for this question