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How do you find the molecular mass when you have STP and density?
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ā 11y ago
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ā 11y ago
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Why is it important to know the mass and volume of gas at STP?
To find it's density
How do you you find moles when given the mass and volume?
Density is the amount of mass per given volume, thus the formula for density of an object with a known mass and volume is as follows: ρ=m/V where: ρ - (rho) Density (Kg m-3) m - Mass (Kg) V - Volume (m3)
What's lighter nitrogen or natural gas?
Technically, atomic nitrogen has less mass than a molecule of methane (CH4 = natural gas) with the former having a mass of 14 and the latter a mass of 16.04. However, in nature, nitrogen exists in its molecular form consisting of two nitrogen atoms. Thus, molecular nitrogen has a molecular weight of 28 vs. 16.04 for methane, making a molecule of atmospheric nitrogen heavier than one of methane. This translates into a density difference as follows: N2 density = 1.251 g/L at STP (standard temperature and pressure) CH4 density = 0.717 g/L at STP Final note: "Natural Gas" is not actually 100% methane. It has a variable composition consisting of 70-90% methane, 5-15% ethane (C2H6) and trace amounts of propane, butane, and other gases.
What is the density of neon gas at STP?
The Density of Neon at STP is: a 0.89994 mg/cm-3.
What is the value of gram molecular volume of oxygen at stp?
5600 mL
Why is it important to know the mass and volume of gas at STP?
To find it's density
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.
How do you you find moles when given the mass and volume?
Density is the amount of mass per given volume, thus the formula for density of an object with a known mass and volume is as follows: ρ=m/V where: ρ - (rho) Density (Kg m-3) m - Mass (Kg) V - Volume (m3)
Density of Hydrogen?
Gaseous hydrogen has a density of 0.08988 g/cm. Liquid and solid hydrogen have a density of about 0.07 g/ccAt standard temperature and pressure (stp), hydrogen as a gas has density 0.08988 grams per litre. Hydrogen atoms have atomic mass of 1, and diatomic hydrogen molecules have molecular mass of 2. From this we can tell that hydrogen is the lightest (least dense) element in the periodic table.
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 volume of methane gas at STP?
Problem: Calculate the density of CH4 gas at STP. How to solve the problem: Density is mass over volume. (D = M/V), this is what we need to find. Information you will need: Molecular weight of CH4 = 16.05 g/mol STP = Pressure (P) = 1 atm (unit of pressure) and Temperature (T) à 273 K (unit of temperature) Use the ideal gas law. PV = nRT n = mass/ mw (molecular weight- "The molecular weight is essentially the same thing as the molar mass except that, as the name implies, it refers to molecules rather than just elements. The molar mass and molecular weight is typically given in units of grams per mole." - Answers.com) n = unit of mass V = unit of volume PV = (mass/mw) RT Steps: Re-arrange the ideal gas law equation, so that you get M/V (which is density). Mass/V = mw (molecular weight) x P/ RT Mass/V = (16.05 g/mol) x 1 atm / [0.08206 (L)(atm)/ (mol)(K)] (273 degrees K) Because of the gas law constant, atm (unit of pressure), K (unit of temperature) and mol (numerical unit) cancel out, and we are left with units of grams per L (unit of volume), which is what we want. Thus, our answer will be in units of g/L. Plug the equation into your scientific calculator. I got 7.16 x 10^-1 g/L
What is the density of francium at STP?
The estimated value of the density of francium at STP is 1,87 g/cm3.
The molar mass of a gas can be determined from?
for Apex: can be found easily from the periodic table is the mass of a mole of the gas
What's lighter nitrogen or natural gas?
Technically, atomic nitrogen has less mass than a molecule of methane (CH4 = natural gas) with the former having a mass of 14 and the latter a mass of 16.04. However, in nature, nitrogen exists in its molecular form consisting of two nitrogen atoms. Thus, molecular nitrogen has a molecular weight of 28 vs. 16.04 for methane, making a molecule of atmospheric nitrogen heavier than one of methane. This translates into a density difference as follows: N2 density = 1.251 g/L at STP (standard temperature and pressure) CH4 density = 0.717 g/L at STP Final note: "Natural Gas" is not actually 100% methane. It has a variable composition consisting of 70-90% methane, 5-15% ethane (C2H6) and trace amounts of propane, butane, and other gases.
What is Neon's density at STP?
no
What is the mass of 100 ml of chlorine in grams?
The mass of the Chlorine will depend upon the density of the Chlorine which depends upon the temperature and pressure of the Chlorine. Assuming stp (standard temperature and pressure) the density of Chlorine is 0.0032 g/ml. density = mass / volume → mass = volume × density = 100 ml × 0.0032 g/ml = 0.32 g.
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.
