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At standard temperature and pressure (STP), one mole of an ideal gas occupies 22.4 liters. To find the number of moles in 16.8 liters of xenon (Xe), divide the volume by the molar volume: ( 16.8 , \text{L} \div 22.4 , \text{L/mol} \approx 0.75 , \text{mol} ). Since one mole contains approximately ( 6.022 \times 10^{23} ) molecules, the number of molecules in 16.8 L of Xe is about ( 0.75 \times 6.022 \times 10^{23} \approx 4.5 \times 10^{23} ) molecules.
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How many grams are contained in 168 l of CO2 at stp?
At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. To find the number of moles in 168 liters of CO2, you can divide 168 by 22.4, which gives approximately 7.5 moles. Since the molar mass of CO2 is about 44 grams per mole, you can multiply 7.5 moles by 44 grams/mole to find that 168 liters of CO2 contains approximately 330 grams.
How many moles are contained in 16.8 L of Xe gas at STP?
16,8 L of Xe gas at STP is equivalent to 0,754 moles.
How many molecules are contained in 16.81 of Xe at STP?
To find the number of molecules in 16.81 grams of xenon (Xe) at standard temperature and pressure (STP), first calculate the number of moles using the molar mass of xenon, which is approximately 131.3 g/mol. The number of moles is 16.81 g / 131.3 g/mol ≈ 0.128 moles. Using Avogadro's number (approximately (6.022 \times 10^{23}) molecules/mol), the total number of molecules is 0.128 moles × (6.022 \times 10^{23}) molecules/mol ≈ (7.71 \times 10^{22}) molecules.
How many molecules are contained in 39.0 l of f2 gas at stp?
To find the number of molecules in 39.0 liters of F₂ gas at standard temperature and pressure (STP), we can use Avogadro's law, which states that 1 mole of any gas occupies 22.4 liters at STP. First, we calculate the number of moles in 39.0 liters: ( \text{Moles of F₂} = \frac{39.0 , \text{L}}{22.4 , \text{L/mol}} \approx 1.74 , \text{mol} ). Next, we convert moles to molecules using Avogadro's number ((6.022 \times 10^{23} , \text{molecules/mol})): ( 1.74 , \text{mol} \times 6.022 \times 10^{23} , \text{molecules/mol} \approx 1.05 \times 10^{24} , \text{molecules} ). Thus, there are approximately (1.05 \times 10^{24}) molecules of F₂ gas in 39.0 liters at STP.
How many molecules are in 1 mol of H2 at STP?
At standard temperature and pressure (STP), 1 mole of any substance contains Avogadro's number of molecules, which is approximately (6.022 \times 10^{23}) molecules. Therefore, 1 mole of (H_2) (hydrogen gas) contains (6.022 \times 10^{23}) molecules of (H_2).
How many grams are contained in 168 l of CO2 at stp?
At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. To find the number of moles in 168 liters of CO2, you can divide 168 by 22.4, which gives approximately 7.5 moles. Since the molar mass of CO2 is about 44 grams per mole, you can multiply 7.5 moles by 44 grams/mole to find that 168 liters of CO2 contains approximately 330 grams.
How many moles are contained in 16.8 L of Xe gas at STP?
16,8 L of Xe gas at STP is equivalent to 0,754 moles.
How many molecules are contained in 16.81 of Xe at STP?
To find the number of molecules in 16.81 grams of xenon (Xe) at standard temperature and pressure (STP), first calculate the number of moles using the molar mass of xenon, which is approximately 131.3 g/mol. The number of moles is 16.81 g / 131.3 g/mol ≈ 0.128 moles. Using Avogadro's number (approximately (6.022 \times 10^{23}) molecules/mol), the total number of molecules is 0.128 moles × (6.022 \times 10^{23}) molecules/mol ≈ (7.71 \times 10^{22}) molecules.
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.
How many liters are in 5.4x1024 molecules of nitric oxide at STP?
Using the ideal gas law (PV = nRT), we can calculate the volume of gas at STP. First, we need to convert the number of molecules to moles by dividing by Avogadro's number. Then, we can use the volume of 1 mole of gas at STP, which is 22.4 liters. Calculate V = (5.4x10^24 / 6.022x10^23) * 22.4 to find the volume in liters.
How many hydrogen molecules are in 31.8 L H2(g) at STP?
To find the number of hydrogen molecules, first calculate the number of moles in 31.8 L of H2 at STP using the ideal gas law. Then use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
How many molecules are contained in 39.0 l of f2 gas at stp?
To find the number of molecules in 39.0 liters of F₂ gas at standard temperature and pressure (STP), we can use Avogadro's law, which states that 1 mole of any gas occupies 22.4 liters at STP. First, we calculate the number of moles in 39.0 liters: ( \text{Moles of F₂} = \frac{39.0 , \text{L}}{22.4 , \text{L/mol}} \approx 1.74 , \text{mol} ). Next, we convert moles to molecules using Avogadro's number ((6.022 \times 10^{23} , \text{molecules/mol})): ( 1.74 , \text{mol} \times 6.022 \times 10^{23} , \text{molecules/mol} \approx 1.05 \times 10^{24} , \text{molecules} ). Thus, there are approximately (1.05 \times 10^{24}) molecules of F₂ gas in 39.0 liters at STP.
How many butane molecules are in 22.4 liters of C4H10 gas at STP?
There are 6.02 x 10^23 molecules in one mole of a substance (Avogadro's number). At STP, 22.4 liters of any ideal gas contains 1 mole of gas. Therefore, there are 6.02 x 10^23 butane molecules in 22.4 liters of C4H10 gas at STP.
How many molecules are in 1 mol of H2 at STP?
At standard temperature and pressure (STP), 1 mole of any substance contains Avogadro's number of molecules, which is approximately (6.022 \times 10^{23}) molecules. Therefore, 1 mole of (H_2) (hydrogen gas) contains (6.022 \times 10^{23}) molecules of (H_2).
How many oxygen molecules are in 9.1 L of oxygen gas at STP?
at stp 1 mole of a gas contains 22.4 litres. 9.1/22.4= .40625 moles o2. 1 mole of a gas contains 6.022E23 molecules so .40625 moles x 6.022E23 = 2.4464325E23 molecules, but you have to multiply by two due to it being diatomic, so answer x 2 = 4.892875E23 molecules
How many molecules are in 7.3 L of H2 at STP?
At STP, 1 mole of any gas occupies 22.4 L. So, 7.3 L of H2 corresponds to 7.3/22.4 = 0.3263 mol. Since 1 mol of H2 contains 6.022 x 10^23 molecules, the number of molecules in 7.3 L of H2 at STP would be 0.3263 mol x 6.022 x 10^23 molecules/mol = 1.963 x 10^23 molecules.
How many molecules of ethane are present in 64.28 liters of ethane gas (C2H6) at STP?
at STP 1 mole occupies 22.4 litres. 64.28 / 22.4 is 2.8696428 moles. Multiply this by avagadro's constant (6.022*10^23) gives 1.7281x10^24 molecules
