Mole ConceptHard

Question

Fluorine reacts with uranium hexafluoride UF6 as represented by the following equation.

U(s) + 3F2(g) → UF6(g)

How many fluorine molecules are required to produce 2.0 mg of uranium hexafluoride UF6 from an excess of uranium? The molar mass of UF6 is 352.0 g mol–1.

Options

A.5.13 × 1018
B.1.026 × 1019
C.2.052 × 1019
D.1.026 × 1020

Solution

U + 3F2 → UF6

3 × 6.022 × 1023 molecule 352 g

∴ Number of F2 molecules needed $= \frac{3 \times 6.022 \times 10^{23}}{352} \times 2 \times 10^{- 3} = 1.026 \times 10^{19}$

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