The equilibrium constant K for the reaction `2HI(g) hArr H_(2)(g)+I_(2)(g)` at room temperature is `2.85` and that at `698 K` is `1.4 xx10^(-2)`. This implies

The equilibrium constant, K for the reaction : 2HI (g) hArr H_(2)(g)+I_(2)(g) at room temperature is 2.85 and that of at 698 K is 1.4 xx 10^(-2) . This implies that the forward reaction is

the equiliberium constant K for the reaction 2HI (g) ⇌ H_2 (g) + I_2 (g) at room temperature 300 K is 2.85 and at 698 K is 1.84 xx 10^(-2) . Hence the reason that HI existsas a stable compound at room temperature is because :

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

In the reversible reaction, 2HI(g) hArr H_(2)(g)+I_(2)(g), K_(p) is

In the reversible reaction, 2HI(g) hArr H_(2)(g)+I_(2)(g), K_(p) is

What will be the equilibrium constant at 717K for the reaction 2HI(g) hArr H_2(g) +I_2(g) if K for H_2(g) +I_2(g) hArr 2HI at 717 K is 50.

The equilibrium constant for the reaction, A+B hArr C+D is 2.85 at room temperature and 1.4xx10^(-2) at 698 K . This shows that the forward reaction is

The equilibrium constant for the reaction, A+B hArr C+D is 2.85 at room temperature and 1.4xx10^(-2) at 698 K . This shows that the forward reaction is