The volume of 10.9 mol of helium at STP is 50 litres.
The volume of any gas at STP (standard temperature and pressure) is 22.4 L/mol. The molar mass of helium is 4.0026 g/mol. So, 84.6 grams of helium would be 84.6/4.0026 = 21.1 mol. Therefore, the volume of 84.6 grams of helium at STP would be 21.1 mol * 22.4 L/mol = 472.64 L.
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.
The volume is 695,85 cm3.
The volume is 695,62 cm3.
1 mol of any gas has a volume of 22.4 L at STP
The volume of any gas at STP (standard temperature and pressure) is 22.4 L/mol. The molar mass of helium is 4.0026 g/mol. So, 84.6 grams of helium would be 84.6/4.0026 = 21.1 mol. Therefore, the volume of 84.6 grams of helium at STP would be 21.1 mol * 22.4 L/mol = 472.64 L.
The mass of 43,7 L of helium at STP is 7.8 g.
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.
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.
The volume of 0.44 mol of C2H6 gas at standard temperature and pressure (STP) is approximately 9.9 L. This is based on the molar volume of a gas at STP, which is around 22.4 L/mol.
The molar volume of a gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, the volume of 2 moles of oxygen gas at STP would be 2 moles * 22.4 L/mol = 44.8 L.
The volume is 695,85 cm3.
The volume is 695,62 cm3.
To find the volume of 19.87 mol of NH₄Cl at STP (standard temperature and pressure), we can use the ideal gas law. At STP, 1 mol of gas occupies 22.4 L. Therefore, 19.87 mol of NH₄Cl will occupy 19.87 mol x 22.4 L/mol = 445.888 L.
1 mol of any gas has a volume of 22.4 L at STP
At standard temperature and pressure (STP), the molar volume of a gas is approximately 22.4 L. To find the volume of 150g of ozone (O3) at STP, you would first convert the mass of ozone to moles, then use the molar volume to find the volume.
To calculate the volume of a gas at STP (Standard Temperature and Pressure), you can use the ideal gas law equation: PV = nRT. At STP, the pressure is 1 atm, the temperature is 273 K, and the molar volume of an ideal gas is 22.4 L/mol. Plugging in the values, you can calculate the volume of 1.50 mol of Cl2 at STP.