During an experiment, solid iodine was placed in a sealed container. The container was gradually heated and purple-colored vapors of iodine formed were observed. Describe this system when it reaches phase equilibrium. (10 points)

See explanation

Explanation:

For a chemical system in a state of dynamic equilibrium, the rate of forward reaction is equal to the rate of reverse reaction.

For this system under consideration;

I2(s)⇄I2(g)

When we heat the container, solid iodine is converted into purple coloured iodine vapour.

When equilibrium is achieved in the system, there will be no net change in the amount of solid iodine and iodine vapour present in the system since the rate of forward and reverse reactions are equal for a system in a state of equilibrium.

i do not get it   at all