Answer:
516.77 grams of Argon gas is present
Explanation:
Using the gas formula
PV = nRT
number of moles (n) = mass / molar weight or mass
P = pressure = 3.4 atm
V = volume = 72 L
R = gas constant = 0.082 L atm mol^-1 K^-1
T = temperature = 225 K
MM = molar mass of Ar = 38.984 g/mol
PV = mRT/ MM
m = PV MM / RT
m = 3.4 * 72 * 38.948 / 0.082 * 225
m = 9534.4704 / 18.45
m = 516.77 grams
the mass of Ar gas you have is 516.77 grams.
2.4 x 10²² atoms
<h3>Further explanation</h3>
Atomic mass is the average atomic mass of all its isotopes
In determining the mass of an atom, as a standard is the mass of 1 carbon-12 atom whose mass is 12 amu
So the atomic mass obtained is the mass of the atom relative to the 12th carbon atom
mass single Uranium atom=4.7 x 10⁻²² g
then for 111 mg=0.111 g
Answer:
at first i would like to tell which class
Explanation:
125000 is the answwr
I think it’s C atomic radius and numbers of unshielded protons
