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1 mol of any gas has a volume of 22.4 L at STP
decreases
You have to say which chemical you have 500 liters of. Moles are not a unit of volume, they refer to a specific number (Avogadro's number) of molecules, and different substances have different molecular sizes.
The frequency of collisions is reduced
The ideal gas law could be written to say the P = nRt/v. So gas pressure, P, is affected by n, the number of gas molecules; t, temperature; and v, volume. "R" is a natural constant.
1 mole of gas at STP occupies 22.4 liters.
1 mole of gas at STP occupies 22.4 liters.
1 mol of any gas has a volume of 22.4 L at STP
1 mole of gas at STP occupies 22.4 liters.
1 mole of gas at STP occupies 22.4 liters.
1 mole of gas at STP occupies 22.4 liters.
decreases
They have an inverse relationship.
First convert the number of grams of CO2 into moles, then use the Ideal Gas Law. For how to solve this problem, see the two Related Questions links to the left of this answer.
You have to say which chemical you have 500 liters of. Moles are not a unit of volume, they refer to a specific number (Avogadro's number) of molecules, and different substances have different molecular sizes.
gas should not freez under normal conditions. i would say that you prob have some bad gas with water in it. i would suggest that u pull it in a garage and thaw it out and then drain it and buy some stp gas treatmet and put the whole bottle in with some new gas
Boyle found that when the pressure of a gas at constant temperature is increased the volume of the gas decreases.When the pressure is decreased the volume increases.