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If given number of moles volume density and molar volume how do you find the molar mass?
Wiki User
ā 15y ago
Molar mass is the sum of all of its elements' average atomic mass in grams. Such as:
NH4 would be calculated by adding nitrogen's aam (14.007) and hydrogen's aam multiplied by four (1.0079 x 4 = 4.0316). Therefore, ammonium's molar mass would be (14.007+4.0316) 18.039. Rounded to sig figs.
Wiki User
ā 15y ago
Wiki User
ā 13y agoVolume = (mass) divided by (density)
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What is difference between partial molar volume and specific volume?
No. Specific volume is the inverse of density. Molar volume specific volume divided by mols. (i.e. g/(mLxMols)
What is molar and molal volume?
The molar volume at STP(22.4 L/mol) can be used to calculate the molar mass of the gas.
How do you find out the molar mass of a gas given density temperature and pressure?
MolarMass = [density x gas constant x temperature(in kelvin)] / pressure (in atm)
How much space will 2.3 grams of sulfur dioxide take up at standard temperature and pressure?
we first find the number of moles( number of moles= mass/molar mass). the we can find the volume by using the formule( volume=number of moles multiplyd by the molar volume)
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 do you find no of atoms if molar mass and density is given?
This is actually a chemistry question, but I found it in the math section... well anyways you use an equation with avogadro's number. P(density)=(((#atoms)(molar mass))/((avogadro's number)(volume))). You're solving for #atoms so rearrange the equation. You have density, molar mass, and avogadro's number. As for volume, assuming you know what element this is (which you should know from the molar mass even if it's not given), you should be able to compute volume from the unit cell measurements. If you do not know unit cells... I'm not sure.
What is difference between partial molar volume and specific volume?
No. Specific volume is the inverse of density. Molar volume specific volume divided by mols. (i.e. g/(mLxMols)
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 do you find moles of a chemical with density and molar mass?
You need also to know the volume or the mass of the sample.
What is molar and molal volume?
The molar volume at STP(22.4 L/mol) can be used to calculate the molar mass of the gas.
How do you find out the molar mass of a gas given density temperature and pressure?
MolarMass = [density x gas constant x temperature(in kelvin)] / pressure (in atm)
How much space will 2.3 grams of sulfur dioxide take up at standard temperature and pressure?
we first find the number of moles( number of moles= mass/molar mass). the we can find the volume by using the formule( volume=number of moles multiplyd by the molar volume)
Whats the formula for mass?
1 Equivalent = 1 Mole / (number of moles per Eq.) Eq. mass = Molar mass / (number of moles per Eq.) N = Eq. concentration (eq/L) = Molar conc.(mol/L) / (number of moles per Eq.) = M / (mol/eq)
Molar volume of liquid is greater than molar volume of gas. why?
That's not true. The molar volume of a gas is always greater than the molar volume of a liquid. I can't think of any exceptions to this.
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.
What does the term molar volume mean?
The molar volume, symbol Vm,[1] is the volume occupied by one mole of a substance (chemical element or chemical compound) at a given temperature and pressure. It is equal to the molar mass (M) divided by the mass density (ρ). It has the SI unit cubic metres per mole (m3/mol),[1] although it is more practical to use the units cubic decimetres per mole (dm3/mol) for gases and cubic centimetres per mole (cm3/mol) for liquids and solids.
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.
