At standard temperature and pressure (STP), one mole of any ideal gas occupies 22.4 liters. Therefore, a cylinder with a larger volume will contain more gas particles. Consequently, a cylinder with the greatest volume at STP will contain the highest number of gas particles, as the number of moles (and thus particles) increases with volume.
The volume of 10.9 mol of helium at STP is 50 litres.
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.
At standard temperature and pressure (STP), one mole of an ideal gas occupies 22.4 liters. Therefore, to find the volume occupied by 0.685 mol of gas at STP, you can multiply the number of moles by the volume per mole: 0.685 mol × 22.4 L/mol = 15.34 liters. Thus, 0.685 mol of gas occupies approximately 15.34 liters 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).
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.
The gas sample that has the greatest number of molecules is the one with the largest amount of substance, which is measured in moles. At STP (standard temperature and pressure), one mole of any gas occupies a volume of 22.4 liters. Therefore, the gas sample with the largest volume at STP will have the greatest number of molecules.
Two samples of gas at STP containing the same total number of molecules would have equal volumes, as Avogadro's Principle states that equal volumes of gases contain equal numbers of molecules at the same temperature and pressure. Thus, 1 mole of any gas at STP will have the same number of molecules as 1 mole of any other gas at STP.
ANY closed cylinder of 4.0 litre will contain the same number of molecules of ANY gas as the 4.0 liter closed cylinder containing O2 gas at the SAME temperature and pressure, since then the volume only depends on the number of molecules, not on the kind of molecules of the gasses concerned
To determine the number of atoms in 560 cm3 of ammonia at STP (Standard Temperature and Pressure), we first need to calculate the number of moles of ammonia present. The molar volume of a gas at STP is 22.4 L/mol, which is equivalent to 22,400 cm3/mol. Therefore, 560 cm3 is equal to 0.025 moles of ammonia. Next, we use Avogadro's number, 6.022 x 10^23 atoms/mol, to find that there are approximately 1.51 x 10^22 ammonia molecules in 560 cm3 at STP.
Avogadro's law states that equal volumes of gases at the same temperature and pressure contain the same number of molecules. Therefore, at standard temperature and pressure (STP), a given volume of gas will contain the Avogadro number of molecules, which is approximately 6.022 x 10^23.
The molar volume of dry carbon dioxide (CO2) at standard temperature and pressure (STP) is approximately 22.4 liters per mole.
At STP, 1 mole of any ideal gas occupies 22.4 liters. Therefore, 5 liters of NO2 at STP will represent 0.22 moles (5/22.4), and this is the case for any other ideal gas. So, the answer is that 5 liter of ANY ideal gas will have the same number of molecules as 5 liters of NO2.
At standard temperature and pressure (STP), one mole of gas occupies 22.4 liters. Therefore, the volume of 2.00 moles of chlorine (Cl₂) can be calculated by multiplying the number of moles by the molar volume: (2.00 , \text{moles} \times 22.4 , \text{L/mole} = 44.8 , \text{L}). Thus, the volume of 2.00 moles of chlorine at STP is 44.8 liters.
Nitrogen gas at STP is less dense than xenon gas at STP because nitrogen has a lower atomic mass and thus lighter molecules, leading to lower density. Additionally, xenon is a noble gas with a higher atomic mass and larger atomic radius, contributing to its higher density.
It occupies 22.4 L
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.