91Ó°ÊÓ

If a 1.271 -g sample of aluminum metal is heated in a chlorine gas atmosphere, the mass of aluminum chloride produced is \(6.280 \mathrm{~g}\). Calculate the empirical formula of aluminum chloride.

A compound was analyzed and was found to contain the following percentages of the elements by mass: tin, \(45.56 \%\); chlorine, \(54.43 \%\). Determine the empirical formula of the compound.

When \(3.269 \mathrm{~g}\) of zinc is heated in pure oxygen, the sample gains \(0.800 \mathrm{~g}\) of oxygen in forming the oxide. Calculate the empirical formula of zinc oxide.

If cobalt metal is mixed with excess sulfur and heated strongly, a sulfide is produced that contains \(55.06 \%\) cobalt by mass. Calculate the empirical formula of the sulfide.

If 1.25 g of aluminum metal is heated in an atmosphere of fluorine gas, 3.89 g of aluminum fluoride results. Determine the empirical formula of aluminum fluoride.

If \(2.50 \mathrm{~g}\) of aluminum metal is heated in a stream of fluorine gas, it is found that 5.28 g of fluorine will combine with the aluminum. Determine the empirical formula of the compound that results.

A compound used in the nuclear industry has the following composition: uranium, \(67.61 \% ;\) fluorine, \(32.39 \%\). Determine the empirical formula of the compound.

A compound was analyzed and was found to contain the following percentages of the elements by mass: lithium, \(46.46 \%\); oxygen, \(53.54 \%\). Determine the empirical formula of the compound.

A compound has the following percentage composition by mass: copper, \(33.88 \%\) nitrogen, \(14.94 \%\); oxygen, \(51.18 \%\). Determine the empirical formula of the compound.

When lithium metal is heated strongly in an atmosphere of pure nitrogen, the product contains \(59.78 \%\) Li and \(40.22 \%\) N on a mass basis. Determine the empirical formula of the compound.