To identify a diatomic gas (x2), a researcher carried out the following experiment: she weighed
an empty 3.1-l bulb, then filled it with the gas at 1.00 atm and 28.0 °c and weighed it again.
the difference in mass was 3.5 g. identify the gas.

Aluminium

Explanation:

Given data:

Volume = 3.1 L

Pressure = 1.0 atm

Temperature = 28.0 °C (28 + 273.15 = 301.15 K)

Mass = 3.5 g

Identify the gas.

Solution:

First of all we will find the number of moles.

PV = nRT

n = PV/RT

n = 1 atm × 3.1 L / 0.0821 L. atm. K⁻¹.mol⁻¹× 301.15 K

n = 3.1 L. atm / 24.72 L. atm. mol⁻¹

n = 0.13 mol

Now we will find the molar mass.

molar mass = 3.5 g / 0.13 mol

molar mass = 26.9 g/mol

The gas is diatomic so, atomic mass will be half of 26.9 g/mol.

26.9 g/mol / 2 = 13.45 g/mol

The element which has atomic mass closer to the 13.45 is aluminium.

2b2t

explanation:

2b2t

i do not get it   at all