Chemwork consider the changes in entropy which occur in the system and surroundings during phase transitions. mark the true statements (select all that apply.) o when ice melts, energy as heat is absorbed and the entropy of the surroundings decreases o when water freezes, energy as heat is absorbed and the entropy of the surroundings increases. o the entropy of the universe remains constant for a process at equilibrium. o when water condenses, energy as heat is given off and the entropy of the surroundings increases. o δg equals zero for phase transitions at their respective equilibrium temperature and 1 atm pressure. when water evaporates, energy as heat is absorbed by the water and the entropy of the surroundings increases. submit show hints

What do you not know about it

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.

The process is c.convection

Burned piece of steel wool does not gain mass. so only d could be true.