When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. using the equation, mg (s) + 2hcl (aq) imported asset mgcl2 (aq) + h2 (g), if 36.5 g of mg and 2 moles of hcl are supplied, identify the limiting reagent.
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The balanced chemical reaction is:

Mg(s) + 2HCl(aq) = MgCl2(aq) + H2(g)

We are given the amounts of reactants to be used for the reaction. This will be the starting point of the calculations.

36.5 g Mg ( 1 mol / 24.31 g ) = 1.50 mol Mg
2 mol HCl

From the reaction, the mole ratio of the reactants is 1:2. In every 1 mole of magnesium 2 mol of hydrochloric acid is required. Therefore, from the amount supplied the limiting reactant is the hydrochloric acid.

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.