When a mixture of aluminum powder and iron(iii) oxide is ignited, it produces molten iron and aluminum oxide. in an experiment, 5.40 g aluminum was mixed with 18.50 g iron(iii) oxide. at the end of the reaction, the mixture contained 11.17 g iron, 10.20 g aluminum oxide, and an undetermined amount of unreacted iron(iii) oxide. no aluminum was left. what is the mass of the unreacted iron(iii) oxide?

2.53 g

Explanation:

Using law of conservation of mass

total mass of reactant = total mass of product

total mass of reactant = mass of aluminum (Al) + mass of iron(III) oxide ( Fe₂O₃) = 5.40 + 18.5 = 23.9 g

total mass of product = mass of aluminum oxide( Al₂O₃) + mass of iron(Fe) = 11.17 + 10.20 = 21.37 g

unreacted mass of iron(III) oxide = 23.9 - 21.37 = 2.53 g

explanation:

considering the bohr theory, the type of connection that requires the transfer the answer conuldn't be right

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