<h3>The density of H₂ = 0.033 g/L</h3><h3>Further explanation</h3>
In general, the gas equation can be written
where
P = pressure, atm , N/m²
V = volume, liter
n = number of moles
R = gas constant = 0.082 l.atm / mol K (P= atm, v= liter),or 8,314 J/mol K (P=Pa or N/m², v= m³)
T = temperature, Kelvin
n = N / No
n = mole
No = Avogadro number (6.02.10²³)
n = m / MW
m = mass
MW = molecular weight
For density , can be formulated :
P = 327 mmHg = 0,430263 atm
R = 0.082 L.atm / mol K
T = 48 ºC = 321.15 K
MW of H₂ = 2.015 g/mol
The density :
The balanced equation would be
3H2 + N2 ———> 2NH3
Is there meant to be a photo here? there are no options so we can’t answer the question.
Answer: The hydrogen bond will typically form between a hydrogen atom and either a nitrogen, sulfur, or oxygen atom.
I hope that this helps you !
Answer:
7.38 g/cm³ is the density of the metal
Explanation:
In a Face-centered cubic unit cell you have 4 atoms. Also, the edge length is √8×r (r is radius of the atom).
To solve this problem, we need first to calculate the volume of the unit cell and then, with molar mass calculate the mass of 4 atoms. As density is the ratio between mass and volume we can obtain this value.
- <em>Volume of the unit cell</em>
Volume = a³
a = √8×r
(r = 198x10⁻¹²m)
a = 5.6x10⁻¹⁰ m
Volume = 1.756x10⁻²⁸ m³
1m = 100cm → 1m³ = (100cm)³:
1.756x10⁻²⁸ m³× ((100cm)³ / 1m³) =
<h3> 1.756x10⁻²² cm³ → Volume of the unit cell in cm³</h3><h3 />
- <em>Mass of the unit cell:</em>
<em>There are 4 atoms of gold:</em>
4 atoms × (1mol / 6.022x10²³ atoms) = 6.64x10⁻²⁴ moles of gold
As 1 mole weighs 195.08g:
6.64x10⁻²⁴ moles of gold × (195.08g / mol) =
<h3>1.296x10⁻²¹g is the mass of the unit cell</h3><h3 />
- <em>Density of the metal:</em>
1.296x10⁻²¹g / 1.756x10⁻²² cm³ =
<h3>7.38 g/cm³ is the density of the metal</h3>
