Question

To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 5.3-L bulb, then filled it with the gas at 1.30atm and 27.0 ∘C and weighed it again. The difference in mass was 7.9g . Identify the gas. Express your answer as a chemical formula.

Please just an answer or an explanation that is easy to understand, like you would a five year old who has big dreams

Answer 1

Dream big.
Use PV = nRT
You know P, V, R (0.08206) and T (use T in Kelvin = 273+c).

Solve for n.
Then mols = n = grams/molar mass.
YOu know grams and mols, solve for molar mass and look it up on the periodic table. Post your work if you get stuck but explain what you don't understand.

Answer 2

3.57 moles equals n, so i divide 7.9 by that to get grams per mole, which is 2.2. I divide that by 2 to get Hydrogen, but that's wrong

Answer 3

No that's wrong, it's 28, divide 2, get N2

Answer 4

Thank you. Thank you. A lot