Name TA Name DATASHEET - EXP 8 SYNTHESIS AND ANALYSIS OF NICKEL COMPLEX Calculation of percentage yield of hexaminenickel(II) chloride: Molar mass of NiCl2·6H2O = 237.69 g mol-1 Molar mass of Ni(NH3)6Cl2 = 314.0003 g mol-1 Mass of starting material (NiCl2·6H2O) = 6.991 g Theoretical yield of product (Ni(NH3)6Cl2) = g Actual mass of product obtained = 4.11 g % yield of Ni(NH3)6Cl2 = % Theoretical Yield Calculation of Ni(NH3)6Cl2: Percent Yield Calculation for Ni(NH3)6Cl2: EXPERIMENT 8 Synthesis and Analysis of Nickel Complex
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1 g / 237.61 g/mol = 0.0383 mol Show more…
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The synthesis of tris(ethylenediamine)nickel(II) chloride is represented by the following unbalanced equation. Note that the molar masses have been calculated for you. NiCl2·6H2O (aq) + H2NCH2CH2NH2 (aq) → [Ni(H2NCH2CH2NH2)3]Cl2 (s) + H2O (l) Balance the equation shown above. b) If 0.275 mole of NiCl2·6H2O were reacted with 0.788 mole of H2NCH2CH2NH2, how many grams of [Ni(H2NCH2CH2NH2)3]Cl2 (s) should you expect to be formed? (Hint: What is the "theoretical yield") Suppose a student was able to isolate 58.0 g of [Ni(H2NCH2CH2NH2)3]Cl2. What was the mass percentage yield? Show your calculations below.
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