32.5 Grams of NaOH(sodium hydroxide) reacts an excess of CO2( carbon dioxide). 2NaOH(s) + CO2(g)—->Na2CO3(s)+H2O(l) a. What is the theoretical yield of Na2CO3 in grams? 43.1g NaCO3 (need help on how to get that answer) b. If 16.45 g of Na2CO3 is formed, what is the perfect yield? 38.2% ( need help on how to get answer)

So3 that’s what i think

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.