An oxide of a metal $M$ (atomic mass $27$ ) contains $52.94%$ of $M$ by mass (O = 16). Select the correct statement(s).

A $100 g$ of the oxide contain 2.94 mol of O atoms.
BThe empirical formula mass of the oxide is $51$ .
CThe empirical formula of the oxide is $M X_{2} O X_{3}$ .
D $51 g$ of the oxide contain $13.5 g$ of $M$ .

Answer: A, C

Moles in 100 g: M = 1.96, O = 2.94; ratio 0.67 : 1 = 2 : 3, so the formula is M2O3 (formula mass 54 + 48 = 102, not 51). 100 g of oxide has 2.94 mol O. In 51 g of oxide the mass of M is 0.5294 x 51 = 27.00 g, not 13.5 g.

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An oxide of a metal M (atomic mass 27) contains 52.94% of M by mass (O = 16). Select the correct statement(s).

Answer: A, C

More questions on Empirical and molecular formula, percentage composition

An oxide of a metal $M$ (atomic mass $27$ ) contains $52.94%$ of $M$ by mass (O = 16). Select the correct statement(s).