Answer:
Convert the mass of each element to moles using the molar mass from the periodic table. Divide each mole value by the smallest number of moles calculated. Round to the nearest whole number. This is the mole ratio of the elements and is represented by subscripts in the empirical formula.
Explanation:
The result is the molecular formula
The mass in grams of 8.94×10²² formula units of CuF₂ is 15.07 g
<h3>Avogadro's hypothesis </h3>
6.02×10²³ formula units = 1 mole of CuF₂
But
1 mole of CuF₂ = 101.5 g
Thus,
6.02×10²³ formula units = 101.5 g of CuF₂
<h3>How to determine the mass of 8.94×10²² formula units of CuF₂</h3>
6.02×10²³ formula units = 101.5 g of CuF₂
Therefore,
8.94×10²² formula units = (8.94×10²² × 101.5 ) / 6.02×10²³
8.94×10²² formula units = 15.07 g of CuF₂
Thus, 8.94×10²² formula units are present in 15.07 g of CuF₂
Learn more about Avogadro's number:
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The maximum number of moles of Nickel Carbonate (NiCO₃) that can form during a precipitation reaction is 0.025 mol. Hope this helped and have a great day!
Answer:
Aluminum + Nickel(Ii) Nitrate = Nickel + Aluminum Nitrate
Explanation:
