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Vinil7 [7]
1 year ago
15

What would be the mass in grams of 8.94 x 10 22 formula units of copper(II) fluoride, CuF 2

Chemistry
1 answer:
Nadya [2.5K]1 year ago
5 0

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:

brainly.com/question/26141731

#SPJ1

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when atoms react, they often lose, gain, or share electrons to form a more stable version of themselves. for example, alkali met
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<h3></h3><h3>What is periodic table?</h3>

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8 0
1 year ago
Read 2 more answers
Osmium is the most dense element we know of. A 22 g sample of Osmium has a volume of 100 cL. Calculate the density of Osmium in
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Answer:

a. V = 1000 mL

b. Denisty = 0.022 g/mL

Explanation:

a.

First we need to convert the volume of the Osmium into mL. For that purpose we are given the conversion unit as:

1 mL = 0.1 cL

Hence, the given volume of Osmium will be:

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<u>V = 1000 mL</u>

b.

The density of Osmium is given by the following formula:

Density = mass/Volume

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<u>Denisty = 0.022 g/mL</u>

5 0
3 years ago
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