Use the equation to answer the question. H2O(l) + heat ⇄ H2O(g)
A sample of water is at equilibrium at 100°C. Which statement best describes what will happen if liquid water is added to the system?

-More liquid water molecules will change to water vapor until a new equilibrium is reached.
-All of the liquid water molecules that are added will become water vapor.
-More water vapor molecules will change to liquid water until a new equilibrium is reached.
-All of the liquid water molecules that are added will remain liquid water.

I need help on this quick check ASAP!

The answer is 65.3312

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.

Answer///precipitate;

Iam pretty sure that the answer is d