Question

2.38g of Uranium was heated strongly in a current of air. The resulting oxide weighed 2.806 g . Determine the empirical formula of the oxide.(At. mass U=238: O=16)

Answer 1

Mass of oxygen that combined with uranium = 2.806 - 2.38

                                                                       = 0.426

Moles of oxygen = 0.426/16 = 0.026625

Moles of uranium = 2.38/238 = 0.01


Mole ratio: Oxygen = 0.026625/0.01 = 2.66 ≈ 2

                  Uranium = 0.01/0.01 = 1


The formula of Uranium oxide is UO2

Answer 2

Answer:

Explanation:

Mass of oxygen that combined with uranium = 2.806 - 2.38

= 0.426

Moles of oxygen = 0.426/16 = 0.026625

Moles of uranium = 2.38/238 = 0.01

Mole ratio: Oxygen = 0.026625/0.01 = 2.66 ≈ 2

Uranium = 0.01/0.01 = 1

The formula of Uranium oxide is UO2