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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