Answer:
The mole fraction of nitrogen is 0.52
Explanation:
Provided information:
Temperature = 31.2 °C
Pressure = 870.2 mmHg
Volume = 15.1 L
Mass of the mixture = 24.1 g
Mole fraction of nitrogen =?
Process:
Converting pressure:
870.2 / 760 = 1.12 atm
Converting temperature:
31.2 + 273 = 304.2 K
Total moles calculation:
PV = nRT
n = PV/RT
n = 1.12 atm × 15.1 L / 0.0821 L.atm. mol⁻¹.K⁻¹ × 304.2 K
n = 16.9 L.atm. / 25 L.atm. mol⁻¹
n = 0.676 mol
Let x be the number of moles of nitrogen.
Thus, the moles of CO₂ = 0.676 - x
The mass of nitrogen = x mol × 28 g/mol, and for CO₂ the mass = 44 g/mol (0.676 - x)
We have 24.1 = 28x + (29.7 - 44x)
Rearranging gives: 24.1 - 29.7 = 28x - 44x
-5.6 = -16 x
Therefore, x = 0.35
Mole fraction of nitrogen:
Mole fraction of nitrogen = moles of nitrogen / total moles
Mole fraction of nitrogen = 0.35 mol / 0.676 mol
Mole fraction of nitrogen = 0.52
Refer to the attached document for the solution.
No, two atoms that have identical mass numbers can never be considered isotopes of one another. This is due to the fact that for atoms to qualify as isotopes, they must consist of the same number of protons while differing in the number of neutrons. If two atoms share the same mass number, their proton count must also be identical, which implies these atoms cannot be isotopes of each other.
Answer: Rearrange the lone pairs of electrons from the outer atom(s) to create double or triple bonds with the central atom.
Explanation:
