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Formaldehyde's molecular formula is CH2O, and according to the atomic masses of its constituent elements, the gas has a molar mass of 30g/mol. If you have 12.3g of it, then set up a direct proportion where 30/1=12.3/x. Solve for x to get 0.41 moles. Multiply this by the constant of 22.4 liters/mole of any gas at STP, and you get 22.4x0.41=9.184 liters CH2O at STP.
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What volume will be occupied by 132 grams of propane at stp?
This volume is 65,68 L.
How many grams of carbon dioxide will occupy a volume 500.0 ml at STP?
We know that one mole of any gas at STP occupies 22.4 liters of volume. We also know that one mole of carbon dioxide is 44.01 grams of CO2. If there are 44.01 grams of this gas in 22.4 liters at STP, then there will be about 0.98 grams of CO2 in half a liter (500 ml) of the gas at STP.
What is molar volume of hydrogen at stp?
24.5
What volume is occupied by 55 g of methane CH4 (g) at STP?
The easiest way to approach this is to remember molar volume: one mole of every (ideal) gas will occupy 22.4 liters at STP - a gas occupies 22.4 L/mol. Since we know that, we can set up a simple proportion that follows the thought process: if one mole of a gas occupies 22.4 liters (at STP), then 2.88 grams of methane occupies x liters. But before we do that, we have a problem: the measurement given is in the wrong units - it is in grams when molar volume is in moles. Therefore, we first need to convert 2.88 grams of methane to moles. To do this, we need the molar mass of the compound - the sum of all the atomic masses involved. Carbon = 12.0 grams Hydrogen = 1.01 grams × 4 atoms = 4.04 grams ------------------------------------------------------------- Methane = 16.04 grams To convert grams to moles: Grams of substance ÷ Molar mass (in grams) = Moles of substance 2.88 grams CH4 ÷ 16.04 grams CH4 = 0.180 moles CH4 Now we follow through with our proportion: 22.4 L/1 mol = x L/.180 mol x = 4.03 L 2.88 grams of methane occupies 4.03 liters at STP
What volume occupied by 1.50 moles of CH4 at STP is?
The amount of oxygen is 0,067 moles.
What volume will be occupied by 132 grams of propane at stp?
This volume is 65,68 L.
What is the volume of 10 grams of CO2 at STP?
5126 cm3
How many grams of carbon dioxide will occupy a volume 500.0 ml at STP?
We know that one mole of any gas at STP occupies 22.4 liters of volume. We also know that one mole of carbon dioxide is 44.01 grams of CO2. If there are 44.01 grams of this gas in 22.4 liters at STP, then there will be about 0.98 grams of CO2 in half a liter (500 ml) of the gas at STP.
What is the volume of 10.9 mol of helium at STP?
The volume of 10.9 mol of helium at STP is 50 litres.
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.
The volume of 1mole of hydrogen bromide at STP is 22.4 liters The gram-formula mass of hydrogen bromide is 80.9 grams per mole What is the density of hydrogen bromide at STP?
3.61g/L D=m/v
How many grams of methane gas CH4 are contained in a volume of 144 liters at STP?
One mole has amass of 16g.There are 6.428mol.Its mass is 102.85g
What is the volume of 84.6 grams of helium at stp?
4 g of helium occupy 22.414 liters. So, 84.6 g of helium occupy 474.056 liters.
What is the volume of 35.7 g of water?
The volume of 35.7 grams of water = 35.7 cubic centimetres at standard temperature and pressure, (STP). This means a sample at 0Ā°C at a pressure of one atmosphere.
What is molar volume of hydrogen at stp?
24.5
What volume is occupied by 55 g of methane CH4 (g) at STP?
The easiest way to approach this is to remember molar volume: one mole of every (ideal) gas will occupy 22.4 liters at STP - a gas occupies 22.4 L/mol. Since we know that, we can set up a simple proportion that follows the thought process: if one mole of a gas occupies 22.4 liters (at STP), then 2.88 grams of methane occupies x liters. But before we do that, we have a problem: the measurement given is in the wrong units - it is in grams when molar volume is in moles. Therefore, we first need to convert 2.88 grams of methane to moles. To do this, we need the molar mass of the compound - the sum of all the atomic masses involved. Carbon = 12.0 grams Hydrogen = 1.01 grams × 4 atoms = 4.04 grams ------------------------------------------------------------- Methane = 16.04 grams To convert grams to moles: Grams of substance ÷ Molar mass (in grams) = Moles of substance 2.88 grams CH4 ÷ 16.04 grams CH4 = 0.180 moles CH4 Now we follow through with our proportion: 22.4 L/1 mol = x L/.180 mol x = 4.03 L 2.88 grams of methane occupies 4.03 liters at STP
What volume occupied by 1.50 moles of CH4 at STP is?
The amount of oxygen is 0,067 moles.
