2HI (g)rightharpoons H2(g)+I2(g) The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of H2 and I2 are added to the system, the equilibrium constant will be

Question

2HI (g)rightharpoons H2(g)+I2(g) The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of H2 and I2 are added to the system, the equilibrium constant will be (A) 3.2 (B) 1.6 (C) 6.4 (D) 0.8

Tardigrade Admin · Accepted Answer

The value of equilibrium constant remains constant for a given reaction at constant temperature.

Q. 2HI(g)⇋H2​(g)+I2​(g) The equilibrium constant of the above reaction is 6.4 at 300K. If 0.25 mole each of H2​ and I2​ are added to the system, the equilibrium constant will be

3.2

1.6

6.4

0.8

The value of equilibrium constant remains constant for a given reaction at constant temperature.

Q. $2 H I (g) ⇋ H_{2} (g) + I_{2} (g)$
The equilibrium constant of the above reaction is $6.4$ at $300 K$ . If $0.25$ mole each of $H_{2}$ and $I_{2}$ are added to the system, the equilibrium constant will be