What is the density of Radon (Rn) gas at STP (standard temperature and pressure)? How do I solve/set up this problem? Thank you!
brain stalled out
22.4 liters / mol
If it is a perfect gas it is 22.4 moles per liter at STP
molecular mass = 222 grams/mol
so
222 grams/22.4 liter = 9.91 grams/liter
You can convert that to Kg/m^3 or whatever if you chose.
http://hyperphysics.phy-astr.gsu.edu/hbase/kinetic/idegas.html
look under section on Standard temperature and pressure
It is worth remembering that one mole is 22.4 liters at STP because often it is faster than going through P V = n R T
This is helpful thank you!
You are welcome :)
To find the density of radon gas at STP (standard temperature and pressure), you need to know the molar mass of radon and use the ideal gas law equation.
1. Start by finding the molar mass (MM) of radon (Rn). Look up the atomic mass of radon on the periodic table, which is approximately 222 g/mol.
2. Next, recall the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atmospheres, atm)
V = volume (in liters, L)
n = moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin, K)
3. At standard temperature and pressure (STP), the conditions are:
T = 273.15 K
P = 1 atm
4. Now, rearrange the ideal gas law equation to solve for moles (n):
n = PV / RT
Since we are looking for the density, which is mass per unit volume, we don't need to calculate the actual volume. Instead, we can assume a volume of 1 L to simplify the calculation.
5. Substitute the values into the equation:
n = (1 atm * 1 L) / (0.0821 L·atm/mol·K * 273.15 K)
n ≈ 0.0448 mol
6. Finally, calculate the density by dividing the molar mass by the volume (assumed to be 1 L):
Density = MM / Volume = MM / 1 L
Density = 222 g/mol / 1 L
Density ≈ 222 g/L
Therefore, the density of radon gas at STP is approximately 222 g/L.