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weqwewe [10]
3 years ago
11

The volume of the nucleus of a carbon atom is about 9.9 10⁻³⁹. the molar mass of carbon is 12.00 g mol⁻¹. what is the density of

the carbon nucleus?
Chemistry
1 answer:
IrinaVladis [17]3 years ago
3 0

Density is defined as the ratio of mass to the volume.

Density = \frac{Mass}{Volume}        (1)

Since, molar mass of carbon is given i.e. 12.00 g mol^{-1}, determine the mass of carbon, we get

1 amu = 1 g/mol

1 amu = 1.66\times 10^{-24} g

Mass of carbon = 12.00 \times 1.66\times 10^{-24}

= 19.92\times 10^{-24} g

=  1.992\times 10^{-23} g

Now, put the value of mass and volume in formula (1)

Density of carbon nucleus =  \frac{1.992\times 10^{-23} g}{9.9 \times 10^{-39} mL}  

= 0.201 \times 10^{16} g/mL

= 2.01 \times 10^{15} g/mL

Hence, density of carbon nucleus = 2.01 \times 10^{15} g/mL

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The characteristic odor of pineapple is due to ethyl butyrate, a compound containing carbon, hydrogen, and oxygen. Combustion of
gavmur [86]

<u>Answer:</u> The empirical formula for the given compound is C_3H_6O

<u>Explanation:</u>

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

C_xH_yO_z+O_2\rightarrow CO_2+H_2O

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Conversion factor:  1 g = 1000 mg

Mass of CO_2=6.32mg=0.00632g

Mass of H_2O=2.58g=0.00258g

Mass of compound = 2.78 mg = 0.00278 g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

  • <u>For calculating the mass of carbon:</u>

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 0.00632 g of carbon dioxide, \frac{12}{44}\times 0.00632=0.00172g of carbon will be contained.

  • <u>For calculating the mass of hydrogen:</u>

In 18g of water, 2 g of hydrogen is contained.

So, in 0.00258 g of water, \frac{2}{18}\times 0.00258=0.000286g of hydrogen will be contained.

  • Mass of oxygen in the compound = (0.00278) - (0.00172 + 0.000286) = 0.000774 g

To formulate the empirical formula, we need to follow some steps:

  • <u>Step 1:</u> Converting the given masses into moles.

Moles of Carbon =\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{0.00172g}{12g/mole}=1.43\times 10^{-4}moles

Moles of Hydrogen = \frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.000286g}{1g/mole}=2.86\times 10^{-4}moles

Moles of Oxygen = \frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.000774g}{16g/mole}=4.83\times 10^{-5}moles

  • <u>Step 2:</u> Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 4.83\times 10^{-5}mol

For Carbon = \frac{1.43\times 10^{-4}}{4.83\times 10^{-5}}=2.96\approx 3

For Hydrogen  = \frac{2.86\times 10^{-4}}{4.83\times 10^{-5}}=5.92\approx 6

For Oxygen  = \frac{4.83\times 10^{-5}}{4.83\times 10^{-5}}=1

  • <u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of C : H : O = 3 : 6 : 1

Hence, the empirical formula for the given compound is C_3H_{6}O_1=C_3H_6O

3 0
3 years ago
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Answer:

• None of these

Explanation:

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5 0
2 years ago
Calculate the density of chloroform
Rina8888 [55]

Answer: The density of chloroform is 1.47 g/mL

Explanation : Given,

Volume = 40.5 mL

Mass of cylinder = 85.16 g

Mass of cylinder and liquid = 145.10 g

First we have to calculate the mass of liquid (chloroform).

Mass of liquid = Mass of cylinder and liquid - Mass of cylinder

Mass of liquid = 145.10 g - 85.6 g

Mass of liquid = 59.5 g

Now we have to calculate the density of liquid (chloroform).

Formula used:

Density=\frac{Mass}{Volume}

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

Density=\frac{59.5g}{40.5mL}

Density=1.47g/mL

Therefore, the density of chloroform is 1.47 g/mL

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