To identify a diatomic gas (x2), a researcher carried out the following experiment: she weighed an empty 4.1-l bulb, then filled it with the gas at 2.00 atm and 24.0 ∘c and weighed it again. the difference in mass was 9.5 g . identify the gas.

The gas is nitrogen gas N2

Explanation:

Step 1: Data given

Volume of the gas = 4.1L

Pressure = 2.00 atm

Temperature = 24.0 °C

Mass = 9.5 grams

Step 2: Calculate moles of gas

p*V = n*R*T

n = (p*V)/(R*T)

⇒ with p = the pressure of the diatomic gas = 2.00 atm

⇒ with V = the volume of the diatomic gas = 4.1L

⇒ with n = the moles of the diatomic gas = TO BE DETERMINED

⇒ with R = the gas constant = 0.08206 L*atm/mol *K

⇒ with T = the temperature = 24.0 °C = 297 K

n = (2.00*4.1)/(0.08206*297)

n = 0.336 moles

Step 3: Calculate molar mass

Molar mass = mass / moles

Molar mass = 9.5 grams / 0.336 moles

Molar mass = 28 g/mol = X2

X has a molar mass of 14 g/mol

The gas is nitrogen gas N2

the answer is 0.42 is that is an option. this question provides no info