An unknown diatomic gas has a density of 3.164 g/l at stp. what is the identity of the gas?

The identity of the diatomic gas is Chlorine (Cl)

From the question, we are to determine the identity of a gas that has a density of 3.164 g/L at stp.

To determine the identity of the diatomic gas, we will determine the mass of 1 mole of the gas

From the formula

Then,

Mass = Density × Volume

Also, at standard temperature and pressure (STP), 1 mole of any gas will occupy a volume of 22.4 L

∴ Mass of the diatomic gas = 3.164 × 22.4

Mass of 1 mole of the diatomic gas = 70.8736 g

Now, we will determine the atomic mass of the gas

Since, the gas is a diatomic gas,

The atomic mass of the gas =

The atomic mass of the gas = 35.4368 g/mol

The atomic mass of the gas ≅ 35.44 g/mol

This is reasonably close to the atomic mass of chlorine ( At. mass of Cl = 35.453 g/mol)

Hence, the identity of the diatomic gas is Chlorine (Cl)

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The identity of the gas is Cl₂ (chlorine)

Explanation:

STP conditions are:

1 atm → Pressure

273.15 K → T°

So, we must use the Ideal Gas Law to get the moles.

Before that, we will think density as data where 3.164 g of diatomic gas are contained in 1 L of volume.

P.V = n . R . T

1 atm . 1 L = n. 0.082 L.atm/mol.K . 273.15K

1 L.atm / (0.082 L.atm/mol.K . 273.15K) = n

0.0446 mol = n

This quantity of diatomic gas, are 3.164 g so the molar mass will be:

Mass / mol = molar mass

3.164 g / 0.0446 mol = 70.9 g/m

The element (a diatomic molecule), which has that molar mass in the periodic table is the Cl₂.

1 Cl = 35.45 g/m

Cl₂. = 70.9 g/m

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

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