A 1.00 g mixture of H2O and D2O was electrolyzed producing H2(g), D2(g) and O2(g). The H2(g) and D2(g) were then completely reacted with Cl2(g) to produce HCl(g) and DCl(g). The HCl(g) and DCl(g) was then dissolved in 1.000 L of water. Then, a 25.00 mL portion of that 1.000 L solution was reacted completely with AgNO3(aq) to give 0.3800 g of AgCl(s). Calculate the mass % (%w/w) of D2O in the original 1.000 g mixture. Atomic Masses (g/mol): H = 1.008, D = 2.014, O = 16.00, Cl = 35.45, Ag = 107.9
A 1.00 g mixture of H2O and D2O was electrolyzed producing H2(g), D2(g) and O2(g). The H2(g) and D2(g) were then completely reacted with Cl2(g) to produce HCl(g) and DCl(g). The HCl(g) and DCl(g) was then dissolved in 1.000 L of water. Then, a 25.00 mL portion of that 1.000 L solution was reacted completely with AgNO3(aq) to give 0.3800 g of AgCl(s). Calculate the mass % (%w/w) of D2O in the original 1.000 g mixture. Atomic Masses (g/mol): H = 1.008, D = 2.014, O = 16.00, Cl = 35.45, Ag = 107.9
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Chapter21: Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 21.200QP
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A 1.00 g mixture of H2O and D2O was electrolyzed producing H2(g), D2(g) and O2(g). The H2(g) and D2(g) were then completely reacted with Cl2(g) to produce HCl(g) and DCl(g).
The HCl(g) and DCl(g) was then dissolved in 1.000 L of water. Then, a 25.00 mL portion of that 1.000 L solution was reacted completely with AgNO3(aq) to give 0.3800 g of AgCl(s).
Calculate the mass % (%w/w) of D2O in the original 1.000 g mixture.
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