Barium oxide, BaO, is manufactured by decomposition of barium carbonate, BaCO3,

Question

Barium oxide, BaO, is manufactured by decomposition of barium carbonate,

BaCO3, in a furnace: BaCO3(s)BaO(s)+CO2(g)

The heat produced by a furnace maintained at a temperature of 600 K can decompose barium carbonate to barium oxide. The spontaneity of a reaction can be determined from the free energy change for the reaction, G. A reaction is spontaneous when the free energy change is less than zero. A reaction is nonspontaneous when the free energy change is greater than zero. A reaction is in equilibrium when the free energy change is equal to zero.

The free energy change GT at 600 K is equal to 1.4×105J/mol. Calculate the equilibrium constant at 600 K .

Explanation / Answer

Given that Go at 600 K = 1.4×105 J/mol = 140000 J/mol

Relation between Go and equilibrium constant K is

Go = -RT lnK where R = 8.314 J/mol/K

Then,

K = e (- Go/RT)  

= e ( -140000 J/mol / 8.314 x 600)

= 6.48x10-13

K = 6.48x10-13

Therefore, Equilibrium constant at 600 K = 6.48x10-13

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