One mole of ethyl alcohol `(C_(2)H_(5)OH)` was treated with one mole of acetic acid at `25^(0)C` .`(2)/(3)` of the acid changes in to ester at equilibrium.The equilibrium constant for the reaction is

One mole of pure ethyl alcohil was treated with one mole of pure acetic acid at 25^(@)C One -third of the acid changes into ester at equilibrium . The equilibrium constant for the reaction will be:

One mole of ethanol is treated with one mole of ethanoic acid at 25^(@)C . Half of the acid changes into ester at equilibrium. The equilibrium constant for the reaction will be

One mole of ethanol is treated with one mole of ethanoic acid at 25^@C . One -fourth of the acid changes into ester at equilibrium . The equilibrium constant for the reaction will be

When 1 mole of pure ethyl alcohol (C_(2)H_(5)OH) is mixed with 1 mole of acetic acid at 25^(@)C. the equilibrium mixture contains 2//3 mole each of ester and water C_(2)h_(5)OH(l)+CH_(3)COOH(l)hArrCH_(3)COOC_(2)H_(5)(l)+H_(2)O(l) The DeltaG^(@) for the reaction at 298 K is :

The standard emf of a cell having one electron change is found to be 0.591 V at 25^@ C , The equilibrium constant of the reaction is :

5 mole of X are mixed with 3 moles of Y. At equilibrium for the reaction, X + Y rarr Z 2 moles of Z are formed. The equilibrium constant for the reaction will be

4 moles of A are mixed with 4 moles of B. At equilibrium for the raction A+BhArrC+D , 2 moles of C and D are formed. The equilibrium constant for the reaction will be

E_"cell"^@ for the reaction , 2H_2O to H_3O^(+) + OH^(-) at 25^@C is -0.8277 V. The equilibrium constant for the reaction is