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SIZIF [17.4K]
3 years ago
8

The units of density are kg/m2. If the density of a liquid is 760.0 kg/m' what is the specific volume? a) 1.316 x 10 m2/kg b) 1.

316 x 10 m3/kg c) without the molecular weight of the liquid it is impossible to determine the specific volume d) none of the above are correct
Chemistry
1 answer:
zlopas [31]3 years ago
6 0

Answer:

The correct answer is: 1.316 . 10⁻³ m³/kg.

Explanation:

The density (ρ) of a substance is the ratio of its <em>mass (m)</em> to its <em>volume (V)</em>. At constant temperature and pressure, its value is constant and it is an intrinsic property of materials. The units of density are kg/m³.

\rho = \frac{m}{V}

The specific volume (ν) of a substance is the ratio of its <em>mass</em> to its <em>volume</em>. We can see that it is the reciprocal of density and an intrinsic property of matter as well. Therefore, the units of specific volume are m³/kg.

\nu = \frac{V}{m}=\frac{1}{\rho }

Given we know the density of the liquid, we can use this relationship to find out its specific volume:

\nu =\frac{1}{\rho }=\frac{1}{760.0kg/m^{3} } =1.316 .10^{-3} m^{3} /kg

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A 1.000 g sample of nitrogen combined with a 0.0720 g sample of hydrogen to form N2H2. What compound is formed if 1.000 g of nit
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Answer:

N₂H₆

Explanation:

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Hence the chemical formula of new compound will be

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An unknown compound contains only carbon, hydrogen, nitrogen, and oxygen. Complete combustion of a 2.77 g sample of the compound
alisha [4.7K]

The molecular formula of the unknown compound is determined as  C₉H₁₁NO₂.

<h3>Molecular formula of the compound</h3>

The molecular formula is calculated as follows;

CHNO  +  O₂ ------------> CO₂  + H₂O

Mass of carbon, C:  = (6.64 x 12)/44 = 1.81 g in 2.77 g sample

Mass of hydrogen, H: = (1.67 x 2)/18 = 0.186 g in 2.77 g sample

Mass of Nitrogen, N: = (2.77 x 0.143)/1.69 = 0.234 g

Mass of oxygen, O:  = 2.77 g - 1.81 g - 0.186 g - 0.234 g = 0.54 g

<h3>molar ratio of the elements: </h3>

C = 1.81 g = 0.15 mol

H = 0.186 g = 0.186 mol

N = 0.234 g = 0.017 mol

O = 0.54 g = 0.0337 mol

divide through with the smallest number of moles (0.017 mol);

C = 9

H = 11

N = 1

O = 2

Molecular formula = C₉H₁₁NO₂

Check the molar mass of the compound = (9 x 12) + (11 x 1) + (14) + (2 x 16) = 165 g/mol

Thus, the molecular formula of the unknown compound is determined as  C₉H₁₁NO₂.

Learn more about molecular mass here: brainly.com/question/21334167

#SPJ1

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2 years ago
Help with 5b. Full explanation please
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Not elementary school work
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