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andrey2020 [161]
2 years ago
12

The Density of pure carbon in Diamond form is 3.52 g/cm^3. How many cubic inches would 23.7 moles of pure diamond occupy?

Chemistry
1 answer:
Vedmedyk [2.9K]2 years ago
5 0

Answer : The volume of pure diamond is 0.493inch^3

Explanation : Given,

Density of pure carbon in diamond = 3.52g/cm^3

Moles of pure diamond = 23.7 moles

Molar mass of carbon = 12 g/mol

First we have to calculate the mass of carbon or pure diamond.

\text{ Mass of carbon}=\text{ Moles of carbon}\times \text{ Molar mass of carbon}

Molar mass of carbon = 12 g/mol

\text{ Mass of carbon}=(23.7moles)\times (12g/mole)=284.4g

Now we have to calculate the volume of carbon or pure diamond.

Formula used:

Density=\frac{Mass}{Volume}

Now putting all the given values in this formula, we get:

3.52g/cm^3=\frac{284.4g}{Volume}

Volume = 80.8cm^3

As we know that:

1cm^3=0.061inch^3

So,

Volume = 0.061\times 80.8inch^3

Volume = 0.493inch^3

Therefore, the volume of pure diamond is 0.493inch^3

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A second-order reaction has a rate law: rate = k[a]2, where k = 0.150 m−1s−1. If the initial concentration of a is 0.250 m, what
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Rate law for the given 2nd order reaction is:

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