Question

$2HI\left(g\right)\rightleftharpoons H_2\left(g\right)+I_2\left(g\right)$
The equilibrium constant of the above reaction is $6.4$ at $300K$. If $0.25mole$ each of $H_2$ and $I_2$ are added to the system, the equilibrium constant will be:

• A. $0.8$
• B. $3.2$
• C. $1.6$
• D. $6.4$

Answer 1

The correct option is D $6.4$

$2HI\left(g\right)\rightleftharpoons H_2\left(g\right)+I_2\left(g\right)$
The equilibrium constant of the above reaction is $6.4$ at $300K$. If $0.25mole$ each of $H_2$ and $I_2$ are added to the system, the equilibrium constant will be 6.4.
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.