A student performed an experiment to determine the empirical formula of aluminum chloride. In this experiment, 1.800 g of aluminum (Al) reacted completely with an excess aqueous HCl to produce 8.894 g of aluminum chloride. a) What is the mass of Al in the aluminum chloride formed during the reaction? b) Determine the mass of Cl in the aluminum chloride formed during the reaction. c) Determine the empirical formula of AlxCly. The molar mass of Al is 26.98 g/mol; that of Cl is 35.45 g/mol. d) Calculate the mass percent of Al and mass percent of Cl in the compound
A student performed an experiment to determine the empirical formula of aluminum chloride. In this experiment, 1.800 g of aluminum (Al) reacted completely with an excess aqueous HCl to produce 8.894 g of aluminum chloride. a) What is the mass of Al in the aluminum chloride formed during the reaction? b) Determine the mass of Cl in the aluminum chloride formed during the reaction. c) Determine the empirical formula of AlxCly. The molar mass of Al is 26.98 g/mol; that of Cl is 35.45 g/mol. d) Calculate the mass percent of Al and mass percent of Cl in the compound
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions
Section: Chapter Questions
Problem 27PS
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A student performed an experiment to determine the empirical formula of aluminum chloride. In this experiment, 1.800 g of aluminum (Al) reacted completely with an excess aqueous HCl to produce 8.894 g of aluminum chloride.
a) What is the mass of Al in the aluminum chloride formed during the reaction?
b) Determine the mass of Cl in the aluminum chloride formed during the reaction.
c) Determine the empirical formula of AlxCly. The molar mass of Al is 26.98 g/mol; that of Cl is 35.45 g/mol.
d) Calculate the mass percent of Al and mass percent of Cl in the compound
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