Which quantity gives the best indication of the relative strength of the hydrogen bonds between the molecules in liquid hydrogen

Answer:

CH4

Explanation:

The ideal behavior of gases generally depends on the strength of intermolecular forces between gas molecules and whether polar bonds are present.

In the case of CCl4, polar bonds exist along with the more electronegative chlorine atom, leading to stronger intermolecular forces at 400K, as opposed to CH4 which contains only non-polar bonds.

Thus, at 400K, CH4 behaves more like an ideal gas compared to CCl4.

Solution:

The molecular formula is PbSO₄, indicating lead sulfate

Option c.

Explanation:

The percentage makeup shows that in 100 g of this compound, there are:

68.3 g of Pb, 10.6 g of S, and (100 - 68.3 - 10.6) = 21.1 g of O

To find the moles of each element, we divide by their molar masses:

68.3 g Pb / 207.2 g/mol = 0.329 moles Pb

10.6 g S / 32.06 g/mol = 0.331 moles S

21.1 g O / 16 g/mol = 1.32 moles O

Next, we find the mole ratio by dividing each by the smallest number of moles:

0.329 / 0.329 = 1 Pb

0.331 / 0.329 = 1 S

1.32 / 0.329 = 4 O

Thus, the molecular formula is PbSO₄, representing lead sulfate.

Answer:

78.96 g of NaC2H3O2

Explanation:

The following information is provided:

• The solution's volume is 350 mL
• The solution's molarity is 2.75 M
• The molar mass of NaC2H3O2 is 82.04 g/mol

We need to find the mass of the solute:

First, we calculate the number of moles:

Moles = Molarity × Volume

Thus;

Moles of solute = 2.75 M × 0.350 L

                        = 0.9625 moles

Next, we find the mass:

Mass = Moles × Molar mass

        = 0.9625 moles × 82.04 g/mol

        = 78.9635 g

      = 78.96 g

Therefore, the amount of NaC2H3O2 required is 78.96 g

Answer: The correct option is (1).

Explanation:

Group 16 is the third-from-last column in the periodic table and is known as the oxygen family.

Members of this group include oxygen, sulfur, selenium, tellurium, and polonium.

Elements in Group 16 have 6 valence electrons in their outermost shell.

The electronic configuration of sulfur is .

Because sulfur belongs to Group 16, it has 6 valence electrons.