We have the following chemical reaction:
[tex]H_2(g)+I_2(g)\rightleftarrows2HI(g)+heat[/tex]
• For this reaction increasing the temperature will shift the equilibrium to the left because it is an exothermic reaction (it releases heat).
• A change in pressure won't affect the equilibrium because the number of moles is the same on each side of the equation.
• Removing HI (the product) will shift the equilibrium to the left whereas adding it will shift it to the right.
• Removing I2 or H2 which are the reactants will shift the equilibrium to the left, whereas adding any of them will shift it to the right.
So, the correct answer is 2: I, VI and VII only.
