DR. CHIRIE SUMANASEKERA
Q2AP-HW_10-30-2017 (Due: 11/3/17)Ch-3 StoichiometryName:__________________________Please answer the questions below in a separate sheet of paper or in the space provided. Show all the steps in your work.Theoretical yieldSilver nitrate, AgNO3 (Molar mass = 169.9 g/mol), reacts with sodium chromate, Na2CrO4 (Molar mass = 161.9 g/mol) to form silver chromate (Molar mass = 331.7 g/mol) and sodium nitrate. If 45.5 ml of 0.2M AgNO3 is mixed with 35.8 ml of 0.436M Na2CrO4, what is (a) the balanced equation for this reaction? (b) What is the theoretical yield of the precipitated silver chromate? (c) How many grams of which reactant are left over?In the reaction, 2AgNO3 + CaCl2 2AgCl + Ca(NO3)2 How many grams of which reactant will remain when a solution containing 20g 2AgNO3 (Molar mass: 170g/mol) is reacted with a solution containing 15g of CaCl2 (Molar mass= 111g/mol)?Titrations:5Fe2+ + MnO4- + 8H+ Mn2+ + 5Fe2+ + 4H2O. How many ml of 0.24 M MnO4- solution will be needed to titrate a 1.56g sample of pure Fe(NO3)2?What is the molarity of an Fe2+ solution if 4.53 ml of an 0.687 M MnO4- solution is required to titrate 30ml of the Fe2+containing solution to the end point?A solution of HCl is titrated with 23.4ml of 0.216 M NaOH. (a) how many grams of HCl were there is the titrated sample? (b) is the volume of the HCl sample is 50ml, what is the molarity of the HCl solution?What is the percent composition of each element in (a) Ca(NO3)2 and (b) CH3CH2NH2? Express your answer in four significant figures.Empirical formulas:A 2.546g sample of a compound was burned in an excess of oxygen. CO2 was collected and weighed 4.98g. the water collected weighed 3.56g. in a separate experiment, 4.738g of a compound was reacted to form 1.79g of Ammonia. What is the empirical formula of this compound?Determine the empirical formula of the following compounds composed of:17.72 g Cl and 3.10g P24.74% K, 40.5% O, 34.76% MnC,H and O that is 40% C, 6.66% H and the rest is Oxygen.Molecular formulas:The following empirical formulas were determined and their molar masses are given in parentheses. Determine the molecular formulas of each one.C3H7 (86 g/mol)CH2 (70 g/mol)C4H3O2 (166 g/mol)C3H7 (86g/mol)BH3 (27.7 g/mol)C4H8O4N4 (76 g/mol) ................
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