A sample weighing 3.071 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3

Question

A sample weighing 3.071 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The Al2O3 does not react. If the sample residue weighs 2.513 g, what is the mass fraction of Fe2O3 in the original sample? answer in form g Fe2O3 over g original sample hint from program: let x be the mass of Fe2O3 in the original sample, and let y be the mass of Al2O3 in the original sample. What is an expression for the mass of the original sample in terms of x and y? How do you write an expression for the mass of the residue in terms of x and y?

Explanation / Answer

"A sample weighing 3.034 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96)" mass Fe2O3 + mass Al2O3 = 3.034 g ===> equation 1 "When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The Al2O3 does not react." Fe2O3 + 3H2 =====>2Fe + 3H2O "The sample residue weighs 2.583 g:" mass Fe + mass Al2O3 = 2.583 g ====> equation 2 ______________________________________

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