100 POINTS! I WILL MARK AS BRAINLIEST FOR FIRST CORRECT ANSWER!!!

When iodine monochloride, ICl, and chlorine gas react in a closed container, the following equilibrium is established:

ICl(l) + Cl₂(g) ⇆ ICl₃(s)

Iodine monochloride, is a brown liquid, whereas chlorine is a yellowish-green gas and ICl₃ is a yellow crystalline solid.
More chlorine is then added to the equilibrium mixture.

a) State what you would observe.
b) What happens to the rate of the forward reaction compared with the backward reaction?
c) What effect does this have on the yield of ICl₃?
d) What happend to the rate of the forward and backward reactions when equilibrium is reached again?

We have that the reaction and a decrease in the concentration of the reactants will favor the reverse reaction that is the decomposition of the yellow iodine trichloride and the formation of green chlorine gas and brown iodine chloride

Given that some green chlorine gas, which is part of the reactant, will be removed, the reverse reaction will be favored and initial concentration of the yellow iodine trichloride and the green chlorine gas will be reduced while the proportional concentration of the brown iodine chloride will increase and the mixture will become more brown.

nevaehmcclure1 nevaehmcclure1 · Answer 2 · 2022-01-13T22:55:11+01:00

nevaehmcclure1 nevaehmcclure1

13-01-2022

Answer:

d because you don't like math or any subject

Answer Link