Answer:
A
Step-by-step explanation:
A
from le chatelier's principle, we know that as the concentration of one reactant or product changes, the equilibrium is shifted. If the concentration of a gaseous or aqueous product increases, the equilibrium is shifted to the left. Iodine is added, which means that the equilibrium is shifted to the left. Iodine increases, and HI increases. Since HI has increased, there must have been some iodine and hydrogen consumed. Since iodine was added, there is a net increase of iodine. However, since hydrogen was consumed and no new hydrogen was added, the concentration of hydrogen decreases