Which of the following gas samples would have the largest volume, if all samples are at the same temperature and pressure? a 0.498 moles CO2
b 19.91 grams of Ar
c They would all have the same volume

They would all have the same volume.

Explanation:

Let us consider the same temperature and pressure of both Ar and CO₂ is standard temperature and pressure.

Standard temperature = 273.15 K

Standard pressure = 1 atm

Number of moles of CO₂ = 0.498 mol

Volume of CO₂ = ?

Solution:

PV = nRT

R = general gas constant = 0.0821 atm.L /mol.K

1 atm × V = 0.498 mol × 0.0821 atm.L /mol.K × 273.15 K

1 atm × V = 11.17 atm.L

V = 11.17 atm.L/1 atm

V = 11.17 L

Volume calculation for Ar:

Number of moles of Ar:

Number of moles = mass/molar mass

Number of moles = 19.91 g /39.95 g/mol

Number of moles = 0.498 mol

Number of moles are same thus it will occupy same volume. We can prove it through calculation given below,

PV = nRT

R = general gas constant = 0.0821 atm.L /mol.K

1 atm × V = 0.498 mol × 0.0821 atm.L /mol.K × 273.15 K

1 atm × V = 11.17 atm.L

V = 11.17 atm.L/1 atm

V = 11.17 L

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons