Finding equilibrium constant and delta g

Question

Assignment:

Question 1. Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below:

N₂(g) + 3H₂(g) → 2NH₃(g)

Given that the standard free energy of formation (ΔGof) of NH₃ (g) is -111 kJ/mol at 335 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.

Question 2. In the previous question, you had to calculate the the standard Free Energy Change (ΔGo) in order to solve for the equilibrium constant, K, for the reaction:

N2(g) + 3H2(g) → 2NH3(g)

This is the Free Energy measured under standard conditions, when the reaction is started with 1.0 M of each of the three gases present. Calculate the non-standard Free Energy change (ΔG) at 298 K, given the following non-standard initial concentrations of the three gases (Answer in kJ).
ΔGfo = -16.6 kJ/mol for NH3 (g) at 298 K

initial concentration (M)
N2    1.0
H2    0.09
NH3    4.1

Provide complete and step by step solution for the question and show calculations and use formulas.