what is the density f 8L of N2 at 25 degreese C at 760 mmhg?
first, find the moles of N2
n=PV/RT
then, the mass=molecularwtN2*n
finally,
density=mass/8 liters
Use P V = n R T
to find n, the number of mols in a liter
(around 1/22.4 moles/liter but the temp is not zero)
then y
N2 weighs 2*14 = 28 grams/mol
so using my 1 mol/22.4 liters
You would have 28 grams/22.4 liters
= 1.25 grams/liter
you probably want grams / cm^3 though.
there are 1000 cm^3 per liter.
so 0.00125 g/cc using my 22.4 liters per mol approx
To find the density of a gas, you need to use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
First, you need to convert the given volume from liters to cubic meters, as the ideal gas law requires the volume to be in SI units. To do this, multiply the given volume by 0.001:
V = 8 L * 0.001 = 0.008 m³
Next, convert the given pressure from mmHg to pascals. The conversion factor is 1 atm = 101,325 Pa:
P = 760 mmHg * (101,325 Pa / 1 atm) = 760 mmHg * (101,325 Pa / (760 mmHg / 1 atm)) = 101,325 Pa
Now, you can substitute the given values into the ideal gas law equation:
PV = nRT
(101,325 Pa) * (0.008 m³) = n * (8.314 J/(mol·K)) * (298 K)
Solving for n (number of moles), you get:
n = (101,325 Pa * 0.008 m³) / (8.314 J/(mol·K) * 298 K)
n ≈ 3.222 moles
Finally, you can calculate the density (ρ) using the formula:
ρ = n / V
ρ = 3.222 moles / 0.008 m³
ρ ≈ 402.75 kg/m³
Therefore, the density of 8 liters of N2 at 25 degrees Celsius and 760 mmHg is approximately 402.75 kg/m³.