2. Reaction is:
N2O4(g) | <--> | 2NO2(g) | |
Initial (bar) | 1 | 0 | |
Change (bar) | - | +2 | |
Equilibrium (bar) | 1- | 2 |
Kp = (PNo2)2 / PN2O4
PN2O4 = xn2O4 P = [(1-) / (1+)]P
and PNO2 = xNO2 P = [2/(1+)] P
Kp = ([2/(1+)] P)2 / ([(1-) / (1+)]P) = 42P / (1-2)
K = 4(0.655)2(1 bar) / (1-(0.655)2) = 3.00 [not 300]
3. As we know
G = -RT ln Kc = -(8.314 J /K.mol * 298.15 K) ln (9.18*10-8) = -40165.93 J/mol = -40.166 kJ/mol
Now,Grxn = G products - Greactants
-40.166 kJ/mol = G(AB2,(aq) ) - G(AB2(s))
-40.166 kJ/mol = G(AB2,(aq) ) - (-152.4kJ/mol)
G(AB2,(aq) ) = 112.2 kJ/mol
From the information in the Data section of the textbook, calculate the equilibrium constant at 3...
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