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Consider the oxidation of a generic metal MM into a metal oxide as shown in the reaction. 2M(s)+2O2(g) M2O4(s)2M(s)+2O2(g) M2O4(s) For this reaction, rxn=4.961 kJ/molrxn=4.961
Consider the oxidation of a generic metal MM into a metal oxide as shown in the reaction.
2M(s)+2O2(g) M2O4(s)2M(s)+2O2(g) M2O4(s)
For this reaction, rxn=4.961 kJ/molrxn=4.961 kJ/mol and rxn=12.12 J/(molK)rxn=12.12 J/(molK) at 298 K.
What is the standard change in Gibbs free energy for the reaction in the forward direction?
rxn= kJ/molkJ/mol
What is the equilibrium constant of this reaction at 298 K?
P=
What is the equilibrium pressure of O2(g)O2(g) over M(s)M(s) at 298 K?
O2= atm
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