If 11g of gas occupies 5.6dm3 at s.t.p calculate it's vapour density (molar volume = 22.4dm3 at s.t.p
To calculate the vapour density of the gas, we need to know the molar mass of the gas. We can use the ideal gas law to find out the number of moles of gas present in the given volume:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
At standard temperature and pressure (STP), P = 1 atm and T = 273 K. We are given that V = 5.6 dm3 and the molar volume of gas at STP is 22.4 dm3. Therefore, the number of moles of gas present is:
n = (PV)/(RT) = (1 atm)(5.6 dm3)/(0.08206 L atm/mol K)(273 K) = 0.229 mol
Next, we can calculate the molar mass of the gas using the given mass and the number of moles:
molar mass = (mass)/(number of moles) = 11 g/0.229 mol = 48 g/mol
Finally, we can calculate the vapour density of the gas, which is defined as the ratio of the molar mass of the gas to the molar mass of hydrogen (which has a vapour density of 1):
vapour density = (molar mass of gas)/(molar mass of hydrogen) = 48 g/mol/2 g/mol = 24
Therefore, the vapour density of the gas is 24.
To calculate the vapor density, we can use the formula:
Vapor Density = (Mass of Gas) / (Molar Volume)
Given:
Mass of gas = 11g
Molar volume = 22.4 dm3 (at s.t.p)
To calculate the vapor density:
Step 1: Convert the mass of the gas to moles using the molar mass.
11g of gas / (molar mass of the gas)
Step 2: Calculate the molar volume of the gas at s.t.p.
Vapor Density = (11g / molar mass of the gas) / 22.4 dm3
Note: The units of the molar mass and molar volume need to be consistent, either in grams or in moles, so make sure to convert them if needed.
I'll need the molar mass of the gas to continue with the calculation.