∆G°=-139kJ/mol.
2SO2(g) + O2(g) → 2SO3(g)
Calculate the Kp at 25 oC for the reaction
Are products or reactants favored at equilibrium? Why?
T= 25.0 oC
= (25.0+273) K
= 298 K
G = -139 KJ/mol
G = -139000 J/mol
we have below equation to be used:
deltaG = -R*T*ln Kc
-139000 = - 8.314*298.0* ln(Kc)
ln Kc = 56.1033
Kc = 2.319*10^24
delta n = number of gaseous molecule in product - number of gaseous molecule in reactant
delta n = -1
Kp= Kc (RT)^delta n
Kp = 2.319*10^24*(0.0821*298.0)^(-1)
Kp = 9.5*10^22
Answer: 9.5*10^22
Since Kp>>1, it is produce favoured
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