2HI-g-rightleftharpoons - H - 2 -g- I - 2 -g-The equilibrium constant of the above reaction is 6-4 300K- If 0-25mole each of -H-2- and -I-2- are added to the system- the equilibrium constant will be-3-20-81-66-4

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The correct option is D 6-42HI-g-x21CC-H2-g-I2-g-The equilibrium constant of the above reaction is 6-4 at 300K- If 0-25mole each of H2 and I2 are added to the system- the equilibrium constant will be 6-4- -xA0-Equilibrium constant depends on temperature and is independent of the actual quantities of reactants and products- the presence of a catalyst and the presence of inert material- It is also independent of concentrations- pressures and volumes of reactants and products-

2HI(g)⇌H2(g)+I2(g)The equilibrium constant of the above reaction is 6.4 at 300K. If 0.25mole each of H2 and I2 are added to the system, the equilibrium constant will be:3.20.81.66.4

$2 H I (g) ⇌ H_{2} (g) + I_{2} (g)$
The equilibrium constant of the above reaction is $6.4$ at $300 K$ . If $0.25 m o l e$ each of $H_{2}$ and $I_{2}$ are added to the system, the equilibrium constant will be:
$3.2$
$0.8$
$1.6$
$6.4$