At `445^(@)C,K_(c)` for the following reaction is `0.020`.
`2HI(g)H_(2)(g)+l_(2)(g)`
A mixture of `H_(2),I_(2)` and `HI` in a vessel at `445^(@)C` has the following concentration: ltbgt `[HI]=2.0M,[H_(2)]=0.50M` and `[I_(2)]=0.10M`. The statement that is true concerning the reaction quotient, `Q_(c)` is:

At 445^(@)C,K_(c) for the following reaction is 0.020 . 2HI(g)rarrH_(2)(g)+I_(2)(g) A mixture of H_(2),I_(2) and HI in a vessel at 445^(@)C has the following concentration: [HI]=2.0M,[H_(2)]=0.50M and [I_(2)]=0.10M . The statement that is true concerning the reaction quotient, Q_(c) is:

Equilibrium concentration of HI, I_(2) and H_(2) is 0.7, 0.1 and 0.1 M respectively. The equilibrium constant for the reaction, I_(2)+H_(2)hArr 2HI is :

Equilibrium concentration of HI, I_(2) and H_(2) is 0.7, 0.1 and 0.1 M respectively. The equilibrium constant for the reaction, I_(2)+H_(2)hArr 2HI is :

In the 500 ml flask following reaction takes place H_(2)(g)+I_(2)(g)hArr 2HI(g) . At equilibrium, concentration of H_(2),I_(2) and HI is 3, 2 and 1.5 mole then the value of K_(C) will be

In the 500 ml flask following reaction takes place H_(2)(g)+I_(2)(g)hArr 2HI(g) . At equilibrium, concentration of H_(2),I_(2) and HI is 3, 2 and 1.5 mole then the value of K_(C) will be

Reaction quotient: At a very high temperature, K_c=65.0 for the following reversible reaction: 2HI(g)hArr H_2(g)+I_2(g) The following concentrations were detected in a mixture. C_(HI)=0.50M , C_(H_2)=2.80M , and C_(I_2)=3.40M Is the system at equilibrium ? If not, in which direction must the reaction proceed for equilibrium to be established?

For these reactions, I H_2(g)+I_2(g) iff 2HI(g)K_c II 2HI(g) iff H_2(g)+I_2(g) :k_c K_C and K_c^' are related as

At 500 K, equilibrium constant, K_(c ) , for the following reaction is 5. (1)/(2)H_(2)(g)+(1)/(2)I_(2)(g)hArr HI(g) What would be the equilibrium constant K_(c ) for the reaction 2HI(g)hArr H_(2)(g)+I_(2)(g)