# Chemistry Stoichiometry Part 2

 Mass from Volume Calculate the mass of N2 needed to produce 43.2 liters of N2O4 when N2 combines with an excess of O2 at STP. Given: MN2 = ?  VN2O4 = 43.2LEquation: Mu = Formula Mass: N 2*14.007 = 28.014Work: 5.40*101g of N2 Volume from Mass Calculate the volume of N2 needed to produce 95.1 g of N2O5 when N2 combines with an excess of O2 at STP. Given: vN2 = ? mN2O5 = 95.1gEquation: Vu = Formula mass: N 2*14.007 + O 5*15.999 = 108.009Work: 1.97 * 101 L of N2 Volume from Volume Calculate the volume of O2 needed to produce 74.1 liters N2O when N2 combines with an excess of N2 at STP. given: vN2O = 74.1L, vO = ?equation: Vu = Work: 74.1 * 1/2 = 3.71 * 101L Mols from Mols Calculate the number of mols of N2 needed to produce 5.25 mols of ammonia when N2 combines with an excess of H2. Given: nN2 = ?, nNH3 = 5.25equation: Work: Nu = 5.25*1/2 = 2.63 * 100 mols Mass from Mols Calculate the mass of N2 needed to produce 4.23 mols of NO2 when N2 combines with an excess of O2. Given: mN2 = ?, nNO2 = 4.23equation: Formula Mass: N 2*14.007 = 28.014Work: 4.23*1/2 *28.014 = 5.928*101g of N2 Mass from Mass Calculate the mass of FeS needed to produce 284g of FeCl2 when FeS combines with an excess of HCl. Given: mFeS = ?, mFeCl2 = 284gEquation: Work: 284/126.751 *1 *87.911 = 1.97*102g Percent Yield Calculate the mass of Ag produced when 150g of AgCl are reacted with an excess of Zn. if the lab reaction only produced 63g of Ag what is the percent yield? given: mAg = ?, mAgCl = 150g, PY = 63gEquation: 150/143.321 * 2/2 * 107.868 = 1.1*102gPercent Yield Equation: PY = Actual/theoreticalWork: 63/110Percent Yield: 57.3% AuthorHenri93 ID267767 Card SetChemistry Stoichiometry Part 2 DescriptionChemistry Stoichiometry Part 2 Updated2014-03-25T00:14:50Z Show Answers