4. Compound X [C16H18N,SCI] was recently synthesized in the laboratory. Your goa

Question

4. Compound X [C16H18N,SCI] was recently synthesized in the laboratory. Your goal is to use spectroscopic analysis of the compound to determine the percent yield for the reaction (similar to the technique used in the Grignard synthesis of Crystal Violet). Using the calibration curve derived from a standard solution of Compound X (shown below) answer the following questions: Absorbance 3 3 3 y = 904x - 0.0196 R? = 0.9987 0,2 0.00E+00 2.50E-04 5.00E-04 7.50E-04 1.00E-03 1.25E-03 1.50E-03 Concentration (M) a.) If a prepared solution of Compound X gave an absorbance of 0.594, determine the molarity of the diluted solution. b.) If the Compound X solution was prepared in the same fashion as in the Grignard experiment (dilution factor = 2000; stock solution volume = 0.010 L), determine the grams of pure Compound X in the synthesized sample. c.) If the theoretical yield for the synthesis of Compound X was 10.25 g, calculate the percent yield for the reaction.

Explanation / Answer

a) From the graph,

Absorbance of 0.594 has the corresponding molarity of 6.50E-04 M

b)molarity of X=6.50E-04 mol/L

molarity of stock* volume of stock=molarity of X* vol of X

molarity of stock=molarity of X* (volume of X/ vol of stock)

Dilution factor=(vol of X/vol of stock)=2000

so ,vol of X=0.010L *2000=5*10^-6 L=20 L

Thus, mol of X=molarity *volume=(6.50E-04 mol/L)*(20L)=0.013 mol

mass of X=mol of X*molar mass of X

molar mass of X(C16H18N3SCl)=16*(12.01g/mol)+(1.008g/mol)*18+3*(14.0g/mol)+32.0g/mol+35.45 g/mol=319.754 g/mol

mass of X=mol of X*molar mass of X=(0.013 mol)*(319.754 g/mol)=4.157 g

mass of X=4.157g

c) % yield=(experimental yield)/theoretical yield)*100=(4.157/10.25)*100=40.5%

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