2. The formula of a compound of lead (Pb) and sulfur (S) was determined using the method in this module. A sample of Pb was weighed into a crucible and covered with finely powdered S. The crucible was covered and heated to allow the Pb and S to react. Additional heating burned off all unreacted S. The crucible was then cooled and weighed. The following data were collected. (a) Calculate the mass of Pb reacted. (b) Calculate the mass of compound that formed. (c) Calculate the mass of S reacted. CHEMISTRY 133 I SUFFOLK COUNTY COMMUNITY COLLEGE (d) Calculate the number of moles of Pb reacted. (e) Calculate the number of moles of S reacted. (f) Find the simplest whole-number ratio of the number of moles of Pb to the number of moles of S in the compound formed. (g) Write the empirical formula for the compound formed. 3. Briefly answer the following questions regarding the experiment described in this module. (a) How high above the inner blue cone of the burner flame should the crucible be when the Mg is heated? (b) What should you do if you see white smoke rising from the crucible in the early stages of heating the Mg ? (c) How will you know when the reaction between Mg and O2 is complete