Consider the decomposition of a metal oxide to its elements, where M represents a generic metal Find: -Grxn -K -P(o2) M2O3(s)<----> 2M(s) +3/2O2 (g) M2O3= -6.70 M(s)=0 02=0 Please explain
The given reaction is follows:
M2O3(s)<----> 2M(s) +3/2O2 (g)
And given that M2O3= -6.70 M(s)=0 02=0
Calculate the dG0 as follows:
dG0 = dG0 (products) - dG0 (reactants)
= 2 * dG0 (M)+ 3/2 * dG0 (O2) - * dG0 (M2O2)
= 2*0+3/2*0- (-6.70)
=6.70 KJ/ mole
T = temperature, 298K
R= 8.314 J/ mol .K
K = exp (-dG0/RT)
= exp - 6.70 *1000J/ mole/8.314 J/ mol .K *298K
=exp-2.70
= 0.0672
Now calculate P(o2) as follows:
K = p (O2)^3/2
0.0672 = p (O2) ^3/2
Now taking log
log 0.0672 = 3/2 log p (O2)
-1.173*2/3= log p (O2)
p (o2)=10^-0.782
= 0.165 atm
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