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Oh, dude, at STP (Standard Temperature and Pressure), one mole of any gas occupies 22.4 liters. So, to find the volume of 55 grams of methane (CH4), we first need to convert grams to moles using the molar mass of methane. Then, we can use the ideal gas law to calculate the volume. It's like a math problem wrapped in a science joke!
At STP (standard temperature and pressure), the volume occupied by 1 mole of any ideal gas is 22.4 L. The molar mass of methane (CH₄) is 16 g/mol. Therefore, 55 g of methane is approximately 3.44 moles. Thus, the volume occupied by 55 g of methane at STP is around 78.4 L.
To calculate the volume occupied by 55 g of methane (CH4) at STP (Standard Temperature and Pressure), we first need to determine the number of moles of methane. The molar mass of methane is 16 g/mol. Therefore, 55 g of methane is equal to 55 g / 16 g/mol ≈ 3.44 mol. At STP, 1 mol of any gas occupies approximately 22.4 L. Therefore, 3.44 mol of methane would occupy approximately 3.44 mol x 22.4 L/mol ≈ 77.1 L.
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
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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
38.0 g F2 = 1.00 mole F2 (divide 38.0 by molar mass= 2*19.00 g/mol)
At STP each (1.00) mole of ANY gas will occupy 22,4 Litre.
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What volume occupied by 1.50 moles of CH4 at STP is?
1 mole of gas at STP (Standard Temperature and Pressure) occupies 22.4 L. Therefore, 1.50 moles of CH4 at STP would occupy 33.6 L (1.50 moles x 22.4 L/mol).
How many molecules are in 30 liters of methane (CH4) at STP?
At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. So, in 30 liters of methane, there would be 30/22.4 = 1.3393 moles. One mole of methane contains 6.022 x 10^23 molecules, therefore 30 liters of methane at STP would contain 1.3393 * 6.022 x 10^23 = 8.07 x 10^23 molecules.
What is the volume in milliliters of 0.0100 mol of ch4 gas at stp?
The volume of 0.0100 mol of CH4 gas at STP (Standard Temperature and Pressure) is 224 mL. This is based on the ideal gas law and the molar volume of a gas at STP, which is 22.4 L/mol. Converting this to milliliters gives 224,000 mL/mol.
How many moles of methane CH4 are present in 5.6L of the gas at STP?
At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. Therefore, 5.6 liters of methane is equal to 5.6/22.4 = 0.25 moles of methane.
What is the volume in liters of 0.75 mol of methane gas (CH4)?
The molar volume of an ideal gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, 0.75 mol of methane gas would occupy 16.8 liters (0.75 mol x 22.4 L/mol = 16.8 L).
What volume occupied by 1.50 moles of CH4 at STP is?
1 mole of gas at STP (Standard Temperature and Pressure) occupies 22.4 L. Therefore, 1.50 moles of CH4 at STP would occupy 33.6 L (1.50 moles x 22.4 L/mol).
How many grams of methane gas CH4 are contained in a volume of 144 liters at STP?
At STP (standard temperature and pressure), one mole of any gas occupies 22.4 liters. This means that 144 liters of methane gas contain 144/22.4 moles of CH4. Using the molar mass of CH4 (16 g/mol), you can calculate the mass of methane gas in grams.
What volume will 3.56 moles of methane occupy at STP?
This volume is 79,79 litres.
How many molecules are in 30 liters of methane (CH4) at STP?
At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. So, in 30 liters of methane, there would be 30/22.4 = 1.3393 moles. One mole of methane contains 6.022 x 10^23 molecules, therefore 30 liters of methane at STP would contain 1.3393 * 6.022 x 10^23 = 8.07 x 10^23 molecules.
What is the volume in milliliters of 0.0100 mol of ch4 gas at stp?
The volume of 0.0100 mol of CH4 gas at STP (Standard Temperature and Pressure) is 224 mL. This is based on the ideal gas law and the molar volume of a gas at STP, which is 22.4 L/mol. Converting this to milliliters gives 224,000 mL/mol.
How many moles of methane CH4 are present in 5.6L of the gas at STP?
At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. Therefore, 5.6 liters of methane is equal to 5.6/22.4 = 0.25 moles of methane.
What is the volume in liters of 0.75 mol of methane gas (CH4)?
The molar volume of an ideal gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, 0.75 mol of methane gas would occupy 16.8 liters (0.75 mol x 22.4 L/mol = 16.8 L).
How many liters of hydrogen gas are needed to react with CS2 to produce 2.5L of CH4 at STP?
The balanced equation for the reaction between hydrogen gas (H2) and carbon disulfide (CS2) to produce methane (CH4) is: 4H2 + CS2 → 4H2S + CH4. This means that for every 4 moles of hydrogen gas, 1 mole of methane is produced. Since 1 mole of any gas at STP occupies 22.4 liters, you would need 5.6 liters of hydrogen gas to produce 2.5 liters of methane.
What volume will the Cl2 occupy at STP?
At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters. Therefore, a volume of 22.4 liters will be occupied by 1 mole of Cl2 gas at STP.
What is the volume of oxygen occupied by two moles?
The molar volume of a gas at STP (standard temperature and pressure) is 22.4 L/mol. Therefore, the volume occupied by 2 moles of oxygen would be 44.8 L.
What is the volume of 1.42 mol of ammonia at STP?
At standard temperature and pressure (STP), the volume occupied by 1 mole of any ideal gas is 22.4 liters. Therefore, the volume of 1.42 moles of ammonia at STP would be 1.42 * 22.4 liters = 31.808 liters.
What is the volume occupied by 0.25mol of chlorine gas?
The volume occupied by 0.25 mol of any ideal gas at standard temperature and pressure (STP) is approximately 5.6 L. This is based on the molar volume of an ideal gas at STP, which is around 22.4 L/mol.
