A 12.95 g sample of Mo2O3 (s) is converted completely to another molybdenum oxide by adding oxygen. The new oxide has a mass of 13.82 g. Add subscripts below to correctly identify the empirical formula of the new oxide.

Question

Hugo Reese

Chemistry

27 September, 11:27

A 12.95 g sample of Mo2O3 (s) is converted completely to another molybdenum oxide by adding oxygen. The new oxide has a mass of 13.82 g. Add subscripts below to correctly identify the empirical formula of the new oxide.

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James Weber · Answer 1

(18.75 g Mo2O3) x [ (1 mole Mo2O3) / (239.88 g) ] x [ (2 moles Mo) / (1 mole Mo2O3) ] = 0.1563 moles

We know that Mox = 0.1563 moles

Mo = 15.00 g Mo, which in turn means that there must be (22.50 - 15.00) grams of O or 7.50 g O, which converts to:

(7.50 g O) x [ (1 mole O) / (15.999 g O) ] = 0.4688 moles O

Taking the ratio of Mo to O results in:

O/Mo = [ (0.4688) / (0.1563) ] = 3