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 constants for the reaction, A_2hArr2A A at 500K and 700K are 1xx10^(-10) and 1xx10^(-5) . The given reaction is

The equilibrium constants for the reaction, A_2hArr2A A at 500K and 700K are 1xx10^(-10) and 1xx10^(-5) . The given reaction is

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 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 at 698 K is 1.4 xx10^(-2) . This implies

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 constants for the reaction, Br_2 hArr 2Br at 500 K and 1xx10^-10 and 1xx^-5 respectively. The reaction is:

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