Question

2.38 gram of uranium was heated strongly in a current of air the resulting oxide weighed 2.806 gram . Determine the empirical formula. of the oxide

Answer 1

Calculations:

Mass of oxygen : 2.806 - 2.38 = 0.426g

Mass of Uranium = 2.38g

Moles of uranium = 2.38 / 238 = 0.01 moles

Moles of Oxygen = 0.426 / 16 = 0.02663 Moles

Mole ratio :

Divide by the smallest mole.

0.02663 / 0.01 = 2.663

0.01 / 0.01 = 1

U : O
1 : 2.663

Rounding off to whole numbers we have.

1 : 3

The emperical formula of the oxide is thus :

UO₃

Answer 2

answer- UO3

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