TWO QUESTIONS I KEEP GETTING WRONG PLEASEEEE HELP!

1)Calculate ΔG (in kJ) at 65 oC for the reaction:

N2O(0.0020 atm) + H2(0.50 atm) ↔ N2(586.9 atm) +H2O(l)

2)Assume that the ΔHo and ΔSo of vaporization do not change significantly with temperature. Calculate the vapor pressure of CH3OH at 43 oC (in atm).

CH3OH (l) ↔ CH3OH(g) . . . ΔHo = 38.0 kJ and ΔSo = 112.9 J/K

Question

TWO QUESTIONS I KEEP GETTING WRONG PLEASEEEE HELP! 

1)Calculate ΔG (in kJ) at 65 oC for the reaction:

N2O(0.0020 atm) + H2(0.50 atm) ↔ N2(586.9 atm) +H2O(l)

2)Assume that the ΔHo and ΔSo of vaporization do not change significantly with temperature. Calculate the vapor pressure of CH3OH at 43 oC (in atm).

CH3OH (l) ↔ CH3OH(g) . . . ΔHo = 38.0 kJ and ΔSo = 112.9 J/K

anonymous · Answer

$$\Delta G = \Delta G°_{f} + RTlnQ$$

use this

anonymous · Answer

The formation you of N2 with that reaction you can calculate that with standard values at 25°C.

the R = 8.314  constant
the T = absolute value kelvins

Q is the Kp which is $$Q = K_{p}\frac{ [586.9] }{ [0.002][0.50] }$$

make sure its balanced...

anonymous · Answer

THANK YOU SO MUCH!