The balanced chemical equation below shows the reaction between nitrogen (N2) and hydrogen (H2) to form ammonia (HN3). N2 + 3H2 - 2NH3
If 10.0 grams of nitrogen reacts with hydrogen to form 12.0 grams of ammonia, then how many grams of hydrogen were used in this
reaction?
A. 2.0 g of H2
o B. 3.0 g of H2
O C. 10 g of H2
OD. 12 g of H2

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.

It must be measured in k.hope my answer is to you : )