What is the mass of radon if its density is 9.73 g/l at stp
at STP, a mole of gas occupies 22.4 L
To determine the mass of radon, given its density at STP (Standard Temperature and Pressure), we need to consider the molar mass of radon and the relationship between density, molar mass, and volume.
1. Look up the molar mass of radon (Rn). The molar mass of radon is approximately 222 g/mol.
2. Use the relationship between density, molar mass, and volume:
Density = mass / volume
3. Convert the given density from g/L to g/cm³, since the molar mass is typically given in g/mol and the volume needs to be in cm³.
1 L = 1000 cm³
Therefore, density = 9.73 g/L = 9.73 g / (1000 cm³)
4. Rearrange the formula to solve for mass:
Mass = Density x Volume
In this case, we assume the volume is 1 cm³ (since this is the volume at STP).
5. Substitute the values into the formula:
Mass = 9.73 g / (1000 cm³) x 1 cm³
6. Calculate the mass:
Mass = 0.00973 g
Therefore, the mass of radon at STP with a density of 9.73 g/L is approximately 0.00973 grams.
To find the mass of radon, we need to use the formula:
Mass = Density x Volume.
Since we are given the density of radon at STP (Standard Temperature and Pressure), which is 9.73 g/L, we need to determine the volume.
At STP, the volume of one mole of any gas is 22.4 L. Since we are dealing with radon, which is a noble gas with an atomic mass of 222 g/mol, we can use this information to find the volume of radon corresponding to its molar mass.
Volume = 22.4 L/mol x (1 mol/222 g) x Mass.
By rearranging the formula, we have:
Mass = (Density x Volume) / (22.4 L/mol x 1 mol/222 g)
Since the density is given as 9.73 g/L, and we know the volume at STP is 22.4 L/mol, we can substitute these values into the equation:
Mass = (9.73 g/L x 22.4 L) / (22.4 L/mol x 1 mol/222 g)
By simplifying, we have:
Mass = (9.73 g x 22.4) / (222 g)
Calculating this, we find:
Mass ≈ 0.986 g
Therefore, the mass of radon at STP would be approximately 0.986 grams.