Hydrogen gas has the lowest mass per mole, with a molar mass of approximately 2 grams per mole.
The weight of a mole of an ideal gas depends on the specific gas being considered. The weight is given by the molar mass of the gas, which is typically expressed in grams per mole.
One mole of magnesium will react with two moles of hydrochloric acid to produce one mole of hydrogen gas. At standard temperature and pressure (STP), one mole of any gas occupies approximately 22.4 liters. Therefore, one mole of magnesium will produce 22.4 liters of hydrogen gas at STP.
A mole of anything has the same number of molecules as a mole of anything else. The why comes from the fact that this is the standard definition as agreed by scientists. We have to have standards for things to work. A mole of anything contains an Avagadro number of particles. That number is 6.022 x 1023
At STP (standard temperature and pressure), all gases have the same volume of 22.4 liters per mole regardless of their identity. Therefore, 1.00 mole of each gas would occupy the same volume of 22.4 liters.
There would be 6.022 x 1023 gas paricles in one mole of that gas.
39.95 because that is the molar mass of Argon
1 mole of gas at STP occupies 22.4 liters.
The Universal Gas Constant is 8.314 J/K/Mole
The mole fraction of oxygen gas in air is approximately 0.21. This means that out of every 1 mole of air, 0.21 moles are oxygen gas molecules.
Hydrogen gas has the lowest mass per mole, with a molar mass of approximately 2 grams per mole.
Compressed natural gas
one mole of a substance is described as 6.02x1023 atoms of a substance so if one mole of bromide gas contains 6.02x1023 atoms then bromide gas will contain one mole. your question is a trick question as the gas is stated as containg one mole there fore it contains one mole of bromide atoms
The volume of a mole of any gas at Standard Temperature and Pressure (STP) is approximately 22.4 liters. This is known as the molar volume of a gas at STP and is a standard value used in gas calculations.
The constant for 1 mole of any ideal gas is known as the ideal gas constant, typically denoted as R. Its value is approximately 8.314 J/molβK.
There is one critical piece of information missing in the question, i.e. which gas are we talking about since different gas will have different molecular weight. In addition 1 mole of gas occupies volume of 22.4 dm3 at stp. This is equivalent to 22.4 L or 0.0224 m3 per mole of gas. Assuming the molecular weight of the gas Y is x g/mole, then the general solution is as followed: 2263000 tons of gas Y equal 226300*1016*1000g/(x g/mole)*(0.0224 m3/mole) equal 5.15022592e9/x m3 of gas Y
22.4 L. At STP 1 mole of any gas will always be equal to 22.4 L.