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How do you find out the molar mass of a gas given density temperature and pressure?
Wiki User
ā 12y ago
MolarMass = [density x gas constant x temperature(in kelvin)] / pressure (in atm)
Wiki User
ā 12y ago
Wiki User
ā 14y agoMolar mass = 2mrt/PV+1.1618^10
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How do you calculate density of chlorine relative to air?
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.
How determine density of gas on hedrogen?
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.
How does the molar concentration at Standard temperature and pressure depend upon the identity of the gas?
Molar concentration is defined as the amount of a gas divided by the volume of gas. According to the gas identity, at standard temperature and pressure, even if the amount of the gas is constant, the volume of gas changes. Thus, the molar concentration changes depending on the gas identity.
If the pressure of gaseous chloroform in a flask is 195 mm Hg at 25C and its density is 1.25 gL what is the molar mass of chloroform?
119g
The molar mass of a gas at STP is the density of that gas?
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.
When a mole of gas occupies 22.4 Liters this is known as?
This is the molar volume of an ideal gas at a given temperature and pressure.
What is the density of gas that has a gram molecular mass of 32 grams?
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.
How do you calculate density of chlorine relative to air?
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.
How determine density of gas on hedrogen?
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.
What is the value of density of cold air?
This density (d) totally depends on the temperature (HOW cold is it) and pressure. Then d = M.p/R.T (in g/m3) in which M = (mean) molar mass of air = 0.8*28 +0.2*32= 28.8 g/mol p = pressure in Pa T = temperature in K R = gasconstant= 8.3145 J/mol.K
What would be a faster way to measure 50 g of water?
Depends on what you want to answer. You have the weight already. Volume can be calculated from the density of dissolved molar volume of dissolved components in the water and the ambient pressure and temperature.
What does molar volume mean for a gas?
Molar gas volume is the volume of ONE moel of gas. It only depends on the pressure and temperature, not on the kind of gas. Molar volume at standard temperature and standard pressure is always 22,4 Litres (for any gas)
Is partial molar property is extensive or intensive propert?
It is intensive property...it doesnt depend upon size of system, but only the chemical nature of mixture or solution at given temperature and pressure..
What happens to the pressure as the density of air decreses?
As air density decreases, the pressure it exerts decreases, but the pressure exerted on it increases.Remember the equation:PV=nRTAnd since n=mass/molar mass,P=nRT/D, density and pressure exerted ON the system have an inverse relationship--as one increases, the other decreases
Calculate the density of nitrogen gas, in grams per liter, at STP?
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.
Weight of a given volume of pure vapor or gas compared to the weight of an equal volume of dry air at the same temperature and volume?
PV = nRTAt a given temperature (T), pressure (P), and volume (V), the number of moles of gas is constant. Thus, whichever gas has a higher molar mass will weigh more. Air is composed of mostly Nitrogen gas (N2), Carbon Dioxide (CO2) and Oxygen gas (O2). The molar masses of these are 28, 44, and 32 respectively.If the pure vapor or gas in question is water vapor (H2O), with molar mass 18, then the air will weigh more.
How does the molar concentration at Standard temperature and pressure depend upon the identity of the gas?
Molar concentration is defined as the amount of a gas divided by the volume of gas. According to the gas identity, at standard temperature and pressure, even if the amount of the gas is constant, the volume of gas changes. Thus, the molar concentration changes depending on the gas identity.
