For the reaction `I_(2)(g) hArr 2I(g)`, `K_(c) 37.6 xx 10^(-6)` at 1000K . If 1.0 mole of `I_(2)` is introduced into a 1.0 litre flask at 1000K, at equilibrium

For the reaction : I_(2)(g)hArr 2I(g), K_(c )=37.6xx10^(-6) at 1000 K. If 1.0 mole of I_(2) is introduced into a 1.0 litre flask at 1000 K at equilibrium, then

If 1.0 "mole" of I_(2) is introduced in a 1.0 litre flask at 1000 K(K_(c)=10^(-6)) , which one is correct?

If 1 mole of I_2 is introduced into 1.o litre flask at 1000 K, at equilibrium (K_c = 10^-6) which one is correct ?

K_c for the reaction : 2H_2S(g) hArr 2H_2(g) + S_2(g) is 1xx10^(-6) at 100 K. What is the dissociation of H_2S is 1 mole of H_2S is introduced in a 1.1 L of flask at 1000 K?

The value of K for H_(2)(g)+CO_(2)(g)hArr H_(2)O(g)+CO(g) is 1.80 at 1000^(@)C . If 1.0 mole of each H_(2) and CO_(2) placed in 1 litre flask, the final equilibrium concentration of CO at 1000^(@)C will be

The value of K for H_(2)(g)+CO_(2)(g)hArr H_(2)O(g)+CO(g) is 1.80 at 1000^(@)C . If 1.0 mole of each H_(2) and CO_(2) placed in 1 litre flask, the final equilibrium concentration of CO at 1000^(@)C will be

The equilibrium constant for the reaction , H_(2) (g) + CO_(2) (g) hArr H_(2) O (g) + CO (g) is 16 at 1000^(@) C . If 1.0 mole of H_(2) and 1.0 mole of CO_(2) are placed in one litre flask , the final equilibrium concentration of CO at 1000^(@) C is

For the equilibrium H_(2)(g)+CO_(2)(g)hArr hArr H_(2)O(g)+CO(g), K_(c)=16 at 1000 K. If 1.0 mole of CO_(2) and 1.0 mole of H_(2) are taken in a l L flask, the final equilibrium concentration of CO at 1000 K will be