To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.6-L bulb, then filled it with the gas at 1.80 atm and 27.0 ∘C and weighed it again. The difference in mass was 9.5 g . Identify the gas. Express your answer as a chemical formula. View Available Hint(s)

The chemical formula of the gas is .

Explanation:

The difference between the container with gas and empty container is equal to the mass of the gas.

Let the gas be

Mass of the gas = m

Molar mass of diatomic gas = M

Pressure of the gas = P = 1.80 atm

Volume of the gas = V = 4.6 L

Temperature of the gas= T = 27.0 C = 27.0 + 273 K = 300 K

Moles of diatomic gas = n =

Using ideal gas equation:

Atomic mass of the element X =

The element is nitrogen and the diatomic gas is .

im not exactly sure but i think its b!