Question

For the reaction $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$, the equilibrium can be shifted in favour of product by:

• A. increasing the $\left[H_2\right]$
• B. increasing the pressure
• C. increasing the $\left[I_2\right]$
• D. by using the catalyst

Answer 1

Answer: (A), (C)

The correct options are
A increasing the $\left[H_2\right]$
C increasing the $\left[I_2\right]$

For the reaction $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$, the equilibrium can be shifted in favour of product by either increasing the $\left[H_2\right]$ or increasing the $\left[I_2\right]$.
Increasing the concentration of reactants favours the product formation.