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What is the volume occupied by 025 moles of chlorine gas?
This volume is 6,197 399 5 at 25 0C.
What is a volume occupied by 0.02 mole of chlorine gas?
This volume is 0,449 L at 0 0C.
Assumption of kinetic theory of gas?
The volume occupied by gas molecules is negligible when compared to volume occupied by the gas.The collisions between gas molecules-gas molecules and gas molecules-walls of the container are perfectly elastic.
Is volume occupied by one mole of a gas dependent on the molar mass of the gas?
No, the volume occupied by one mole of a gas at a given temperature and pressure is the same for all gases, according to Avogadro's hypothesis and the ideal gas law. This is known as the molar volume of a gas, which is approximately 22.4 liters at standard temperature and pressure (STP).
What volume is occupied of 0.48 moles of hydrogen?
The volume of a gas depends on its pressure, temperature, and volume according to the ideal gas law PV = nRT. Without knowing the pressure, temperature, or container size, it's not possible to determine the volume occupied by the 0.48 moles of hydrogen.
What is the volume occupied by 025 moles of chlorine gas?
This volume is 6,197 399 5 at 25 0C.
What is a volume occupied by 0.02 mole of chlorine gas?
This volume is 0,449 L at 0 0C.
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.
What volume is occupied of 2.4 moles of chlorine?
The volume that 2.4 moles of chlorine gas would occupy depends on the temperature and pressure of the gas, according to the ideal gas law (PV = nRT). At standard temperature and pressure (STP), which is 0°C and 1 atm pressure, 2.4 moles of chlorine gas would occupy approximately 53.75 liters.
Assumption of kinetic theory of gas?
The volume occupied by gas molecules is negligible when compared to volume occupied by the gas.The collisions between gas molecules-gas molecules and gas molecules-walls of the container are perfectly elastic.
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.
Is volume occupied by one mole of a gas dependent on the molar mass of the gas?
No, the volume occupied by one mole of a gas at a given temperature and pressure is the same for all gases, according to Avogadro's hypothesis and the ideal gas law. This is known as the molar volume of a gas, which is approximately 22.4 liters at standard temperature and pressure (STP).
What aspects are not accounted for in the ideal gas law?
The ideal gas law does not account for the volume occupied by gas particles and the interactions between gas molecules.
What volume is contained of 2.4 moles of chlorine and how do you work it out?
I would assume chlorine gas and standard temperature an atmospheric pressure. Using the ideal gas equation. PV = nRT (1 atm)(X volume) = (2.4 moles Cl2)(0.08206 Mol*K/L*atm)(298.15 K) Volume = 59 Liters of chlorine gas --------------------------------------------
What volume is occupied of 0.48 moles of hydrogen?
The volume of a gas depends on its pressure, temperature, and volume according to the ideal gas law PV = nRT. Without knowing the pressure, temperature, or container size, it's not possible to determine the volume occupied by the 0.48 moles of hydrogen.
Is volume liquid?
Volume is the amount of 3-dimensional space occupied by an object. It could be a liquid, but it can also be a gas. For example, a glass of air.
How many liters of 17.32g of chlorine gas can be produced?
To calculate the volume of chlorine gas produced, you need to know the molar mass of chlorine and use the ideal gas law equation. First, convert the mass of chlorine gas to moles using its molar mass. Then use the ideal gas law equation PV = nRT, where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature. Finally, you can solve for V to find the volume in liters.
