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Hatshy [7]
3 years ago
8

How many atoms of carbon (C,12.01 g/mol) are in a diamond with a mass of 0.568 g?

Chemistry
1 answer:
Fantom [35]3 years ago
5 0

2.85 × 10^22. A diamond with a mass of 0.568 g contains

2.85 × 10^22 atoms C.

Diamond is a form of pure carbon.

a) Convert <em>grams of C to moles of C</em>

Moles of C = 0.568 g C × (1 mol C/12.01 g C) = 0.047 29 mol C

b) Convert <em>moles of C to atoms of C </em>

Atoms of C = 0.047 29 mol C × (6.022 × 10^23 atoms C)/(1 mol C)

= 2.85 × 10^22 atoms C

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SOLVE The density of a gas is 0.68 g/mL. What amount of space would 23.8 g of this gas occupy?
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Answer:

<h2>The answer is 35 mL</h2>

Explanation:

Density of a substance can be found by using the formula

Density(\rho) =  \frac{mass}{volume}

From the question we are finding the amount of space the gas will occupy that's the volume of the gas

Making volume the subject we have

volume =  \frac{mass}{Density}

From the question

mass = 23.8 g/mL

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Substitute the values into the above formula and solve

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