4. A constant volume of gas has a pressure of ​98.3 kPa​ at ​497 K​ . Determine the temperature of the gas if the pressure is increased to ​182.5 kPa​ . a) Should the temperature of the gas increase or decrease? b) Using Kinetic Molecular Theory (KMT), explain your answer to (a). ​HINT​: What happens to the particles? c) Determine the final temperature of the gas. P​ 1​= P​ 2​= T​ 1​= T​ 2​= k = k =

The answer to the question is d

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.