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3 years ago

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Chemistry

2 answers:

EleoNora [17]3 years ago

6 0

Answer: Option (c) is the correct answer.

Explanation:

Molecules of a molecular solid are held together by weak forces like london dispersion forces, dipole-dipole forces.

So, due to weak forces present in these molecules it is easy to break the bond between them. Hence, molecular solids have low melting point.

Whereas in ionic compounds, atoms are held together by strong forces due to the presence of opposite charges on the atoms of the solid.

Therefore, we can conclude that compared with the melting points of ionic compounds, the melting points of molecular solids tend to be lower.

11111nata11111 [884]3 years ago

5 0

Lower

Melting points of molecular solids are lower than melting points of ionic compounds

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A 3.76 g sample of a compound consisting of carbon, hydrogen, oxygen, nitrogen, and sulfur was combusted in excess oxygen. This

boyakko [2]

Answer: The empirical formula is C3H8S2NO.

Explanation: To determine the formula, find the porcentage of mass of each element in the sample:

1) For C (Molar Mass = 12u)

Note: molar mass of CO2 = 44g/mol

1 mol of CO2 = $\frac{4,06}{44}$ = 0,092g/mol

In 1 mol of CO2, 1 mol of C, so mass of C is

mC = 0,092 . 12 = 1,104g

$\frac{mC}{msample}$ . 100 = $\frac{1,104}{3,76}$ . 100 = 29,4%

2) For H (Molar Mass = 1u)

Note: molar mass of H20 = 18g/mol

1 mol of H2O = $\frac{2,22}{18}$ = 0,124 g/mol

In 1 mol of H2O, 2 mols of H, so mass is

mH = 0,124 . 2 . 1 = 0,248g

$\frac{mH}{msample}$ . 100 = $\frac{0,248}{3,76}$ . 100 = 6,6%

3) For S (Molar Mass = 32u)

Note: molar mass of SO3 = 80g/mol

1 mol of SO3 = $\frac{3,73}{80}$ = 0,046g/mol

In 1 mol of SO3, 1 mol of S, so its mass is:

mS = 0,046 . 32 = 1,472g

$\frac{mS}{msample}$ . 100 = $\frac{1,472}{3,73}$ . 100 = 39,5%

4) For N (Molar Mass = 14u)

Note: molar mass of HNO3 = 63g/mol

1 mol of HNO3 = $\frac{4,40}{63}$ = 0,07

In 1 mol of HNO3, 1 mol of N, so the mass is

mN = 0,07 . 14 = 0,98g

$\frac{mN}{msample}$ . 100 = $\frac{0,98}{8,53}$ . 100 = 11,5%

5) For O (Molar Mass = 16u).

O = 100% - (29,4%+6,6%+39,5%+11,5%)

O = 13%

It's determined the porcentage of the composition. Assuming that 100g of the compound, we calculte the mols of each:

Carbon = $\frac{29,4}{12}$ = 2,45 mol

Hidrogen = 6,6 mol

Sulfur = 1,25 mol

Nitrogen = 0,82 mol

Oxygen = 0,81 mol

Divide each by 0,81, the empirical formula of the compound is C3H8S2NO

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