Density is mass per volume. Density of gas is mostly the same in mol/volume. The molecular mass play large role in the different of density. Weak intermolecular force and interaction among different species of gases may give extra additional to the different in density of mix gas but at very small fraction.
STP is standard temperature and pressure. According to Avogadro's Law equal volumes of gases at the same temperature and pressure contains same number of molecules, regardless of their chemical nature and physical properties.
The density of the gas at STP.
NO.
Use the formula PV=nRT
Hydrogen? You need the conditions, pressure and temperature, of the gas. 1 mole of the gas occupies 22.4 liters at STP. The molar mass of hydrogen is 2.0 g/ mole. So the density at STP is 2.0 / 22.4 = 0.0893 g/liter. At any other pressure and temperature you can use the ideal gas law to find the volume of one mole and then find the density.
MolarMass = [density x gas constant x temperature(in kelvin)] / pressure (in atm)
Molar mass of CO2 is 44. Molar mass of NH3 is 17
To calculate the density of chlorine relative to air, you would use the formula: Density relative to air = Density of chlorine gas Density of air at the same conditions Density relative to air= Density of air at the same conditions Density of chlorine gas ā The density of a gas can be calculated using the ideal gas law: Density = Molar mass Molar volume Density= Molar volume Molar mass ā Where: Molar mass is the mass of one mole of the substance (in grams per mole). Molar volume is the volume occupied by one mole of the substance at a particular temperature and pressure. For chlorine gas ( ļæ½ ļæ½ 2 Cl 2 ā ), the molar mass is approximately 70.91 ā g/mol 70.91g/mol. The density of air is typically around 1.225 ā kg/m 3 1.225kg/m 3 at standard temperature and pressure (STP), which is defined as 0 , ^\circ \text{C} (273.15 K) and 1 ā atm 1atm pressure. So, to find the density of chlorine gas relative to air, you would substitute the values into the formula: Density relative to air = ( 70.91 ā g/mol ) ( 1.225 ā kg/m 3 ) Ć ( 1 ā mol 1000 ā g ) Density relative to air= (1.225kg/m 3 ) (70.91g/mol) ā Ć( 1000g 1mol ā ) This calculation will give you the density of chlorine gas relative to air under the specified conditions. Keep in mind that the densities and conditions may vary, and you should use the appropriate values for the specific conditions you are considering.
The molar mass of C3H8 is 44.11g, so 44.11g/22.4L = 1.96g/L I think this is the answer, I'm not sure but I hope this is make you easier :)
At Standard Temperature and Pressure (STP), which is defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere pressure, the molar volume of an ideal gas is approximately 22.4 liters/mol. The molar mass of nitrogen gas (Nā) is approximately 28.02 grams/mol. To calculate the density (D) of nitrogen gas at STP, you can use the ideal gas law: ļæ½ = Molar mass Molar volume at STP D= Molar volume at STP Molar mass ā ļæ½ = 28.02 ā g/mol 22.4 ā L/mol D= 22.4L/mol 28.02g/mol ā ļæ½ ā 1.25 ā g/L Dā1.25g/L Therefore, the density of nitrogen gas at STP is approximately 1.25 grams per liter.
At STP 1 mole of a gas occupies 22.4 L So D = m / V = 1.222g / 22.4 L = 0.0546 g/L This is the mathematical answer, but this is impossible. The lightest gas is Hydrogen with a molar mass of 2. No real gas is less than that.
Hydrogen? You need the conditions, pressure and temperature, of the gas. 1 mole of the gas occupies 22.4 liters at STP. The molar mass of hydrogen is 2.0 g/ mole. So the density at STP is 2.0 / 22.4 = 0.0893 g/liter. At any other pressure and temperature you can use the ideal gas law to find the volume of one mole and then find the density.
To find it's density
The weight of chlorine gas can vary depending on the volume and temperature. At standard temperature and pressure (STP), the molar mass of chlorine gas (Cl2) is approximately 70.91 grams/mol. To convert this to pounds, you would divide the molar mass by the conversion factor of 453.592 grams per pound. Therefore, the weight of chlorine gas would be approximately 0.156 pounds per mol at STP.
MolarMass = [density x gas constant x temperature(in kelvin)] / pressure (in atm)
Molar mass of CO2 is 44. Molar mass of NH3 is 17
To calculate the density of chlorine relative to air, you would use the formula: Density relative to air = Density of chlorine gas Density of air at the same conditions Density relative to air= Density of air at the same conditions Density of chlorine gas ā The density of a gas can be calculated using the ideal gas law: Density = Molar mass Molar volume Density= Molar volume Molar mass ā Where: Molar mass is the mass of one mole of the substance (in grams per mole). Molar volume is the volume occupied by one mole of the substance at a particular temperature and pressure. For chlorine gas ( ļæ½ ļæ½ 2 Cl 2 ā ), the molar mass is approximately 70.91 ā g/mol 70.91g/mol. The density of air is typically around 1.225 ā kg/m 3 1.225kg/m 3 at standard temperature and pressure (STP), which is defined as 0 , ^\circ \text{C} (273.15 K) and 1 ā atm 1atm pressure. So, to find the density of chlorine gas relative to air, you would substitute the values into the formula: Density relative to air = ( 70.91 ā g/mol ) ( 1.225 ā kg/m 3 ) Ć ( 1 ā mol 1000 ā g ) Density relative to air= (1.225kg/m 3 ) (70.91g/mol) ā Ć( 1000g 1mol ā ) This calculation will give you the density of chlorine gas relative to air under the specified conditions. Keep in mind that the densities and conditions may vary, and you should use the appropriate values for the specific conditions you are considering.
To calculate the density of a gas, we need to know the molar mass and the pressure and temperature conditions. Without this information, we cannot determine the density of the gas.
for Apex: can be found easily from the periodic table is the mass of a mole of the gas
The molar mass of C3H8 is 44.11g, so 44.11g/22.4L = 1.96g/L I think this is the answer, I'm not sure but I hope this is make you easier :)
Yes as is the molar mass of anything else.