Mole map practice II Use the balanced equation given to solve the following questions, show your work for full credit even if it is just the key sequence from your calculator or a picture of your work on paper.

Given the following reaction, answer the questions that follow using a mole ratio.

MgCl2 + Cu2S → 2 CuCl + MgS

If you have 3 mols of Cu2S, how many grams of CuCl can you create?

If you have 4.5 g of MgCl2 how many grams of MgS can you create?

Given the following reaction, answer the questions that follow using a mole ratio.

CaS + F2 → CaF2 + S

If you have 2.1 mols of F2 how many grams of S can you create?

Given the following reaction, answer the questions that follow using a mole ratio.

3NiO2 + 4 Al → 2 Al2O3 + 3 Ni

If you have 5.3 g of Al, how many mols of Al2O3 can be made?

If you have 0.098 g of NiO2 how many grams of Ni can you create?

PLEASE HELP!!! ASAP

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.