Identify the correct equation for the equilibrium constant Kc for the reaction given. C u ( s ) + 2 A g N O 3 ( a q ) − ⇀ ↽ − C u ( N O 3 ) 2 ( a q ) + 2 A g ( s ) Cu(s)+2AgNOX3(aq)↽−−⇀Cu(NOX3)X2(aq) +2Ag(s) Select one: K c = [ Cu ( NO 3 ) 2 ] [ Ag ] 2 [ AgNO 3 ] 2 [ Cu ] Kc=[Cu(NO3)2][Ag]2[AgNO3]2[Cu] K c = [ Cu ( NO 3 ) 2 ] 2 [ Ag ] [ AgNO 3 ] [ Cu ] 2 Kc=[Cu(NO3)2]2[Ag][AgNO3][Cu]2 K c = [ Cu ( NO 3 ) 2 ] [ AgNO 3 ] 2 Kc=[Cu(NO3)2][AgNO3]2 K c = [ Cu ( NO 3 ) 2 ] [ AgNO 3 ] Kc=[Cu(NO3)2][AgNO3]

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Given data,temperature, t = 230°c = 503 kconsider the chemical reaction,ch₃oh(l) + 1/2 o₂(g)  → ch₂o(g) + h₂o(l)calculate the enthalpy change for the reaction: δh⁰rxn =  σnδh⁰f(products) -  σmδh⁰f(reactants)substitute the values from the table: δh⁰rxn = { -115.9 + (-285.8)} - {0+(-238.7)}              = -163.0 kjcalculate the entropy change for the reaction.δs⁰rxn = (219 + 70) - (127.2 + 1/2 x 205.2) = 59.2 j/kconsider the expression for free energy: δg⁰rxn =  δh⁰rxn - t  δs⁰rxnsubstitute the values in the above equationδg⁰rxn = -163 x 10³ - (503 x 59.2)              = -192777.6 j              = -192.777 kj