Consider the decomposition of a metal oxide to its elements, where M represents

Question

Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. M2O(s) 2M(s) + 1/2O2(g) Substance delta G degree f (kJ/mol) M2O(s) -10.10 M(s) 0 O2(g) 0 What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? delta G degree rxn = Number kJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? K = Number What is the equilibrium pressure of O2(g) over M(s) at 298 K? PO2 = Number atm

Explanation / Answer

?Gorxn = 10.10 kJ/mol

K = e -10.10/(0.008314472*298) = 0.0176683476 = 0.01767 = 1.767*10-2

P O2 = K2 = 0.0003122 = 3.122*10-4 atm

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