How much zinc is too much?

How to determine the experimental empirical formula of Zinc Chloride?

• What is the experimental empirical formula of zinc chloride? Im stuck on this problem for my lab Determine the simplest whole number ratio of moles of zinc used, to moles of chlorine reacted in the zinc chloride that was produced. (Take your answers to #4 and #5, and divide both values by whatever value is smaller.) This is what i have figured out so far Mass of empty 100ml beacker= 55.45g mass of Zn metal = 1.80g Mass of beaker containing zinc chloride =58.16g 2.71g of zinc chloride produced .91g of chloride reacted .0275 moles of Zn used .0257 moles of Cl used

• Answer:

  i already showed you this in your last question the moles of Zn = 0.0275 the moles of Cl = 0.0257 to find the molar ratio of Zn:Cl, divide each by the smallest number of moles present Zn = 0.0275 / 0.0257 = 1.07 Zn Cl = 0.0257 / 0.0257 = 1 Cl ZnCl is your empirical formula the real empirical and molecular formula = ZnCl2