At a certain temperature the equilibrium constant `K_C` is 0.25 for the reaction `A(g)+B(g)hArrC(g)+D(g)` If we take 1 mole of each of four gases in a 10 litre container , what woluld be the equilibrium concentration of A(g) ?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?

At a certain temperature the equilibrium constant K_c is 0.25 for the reaction A_(2(g))+B_(2(g)) harr C_(2(g))+D_(2(g)) If we take 1 mole of each of the four gases in a 10 litre container, what would be equilibrium concentration of A_(2(g)) ?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g) hArr C_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container, what would be equlibrium concentration of A_(2)(g) ?

At a certain temperature, equilibrium constant (K_(c)) is 16 for the reaction: SO_(2)(g)+NO_(2)(g) hArr SO_(3)(g)+NO(g) If we take 1 mol of each of the four gases in a 1L container, what would be the equilibrium concentrations of NO and NO_(2) ?

At a certain temperature, equilibrium constant (K_(c)) is 16 for the reaction: SO_(2)(g)+NO_(2)(g) hArr SO_(3)(g)+NO(g) If we take 1 mol of each of the four gases in a 1-L container, what would be the equilibrium concentrations of NO and NO_(2) ?

At a certain temperature , the equilibrium constant (K_(c)) is 4//9 for the reaction : CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) If we take 10 mole of each of the four gases in a one - litre container, what would be the equilibrium mole percent of H_(2)(g) ?

At a certain temperature , the equilibrium constant (K_(c)) is 4//9 for the reaction : CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) If we take 10 mole of each of the four gases in a one - litre container, what would be the equilibrium mole percent of H_(2)(g) ?