A mole of an ideal gas at STP occupies one standard molar volume. This is about 22.4 liters. (If you want the exact figure, PV = nRT; n, T, and P are known (1 mole, standard temperature, standard pressure), R is a constant; solve for V.)
One mole of any ideal gas occupies 22.4 liters at STP - this is called molar volume.
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Because water vapor is considered an ideal gas and all ideal gases have a 1 mol: 22.4 L ratio at STP, the volume occupied by 1 mol of water vapor will be 22.4 L.
1g of N2 = 1/28 = 0.036mol. This times 22.4 = 0.81L or 810mL.
The volume is 0,8 L.
molar volume
The volume is 102 mL.
We know that one mole of any gas at STP occupies 22.4 liters of volume. We also know that one mole of carbon dioxide is 44.01 grams of CO2. If there are 44.01 grams of this gas in 22.4 liters at STP, then there will be about 0.98 grams of CO2 in half a liter (500 ml) of the gas at STP.
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
This depends on the temperature and the pressure. At standard temperature and pressure 1 mole will occupy 22.4 L, so multiply... 22.4 x 2.22 = 48.728 L at STP.
0.00922 g of H2 gas will occupy approximately 0.100 L at STP
The volume is approx. 15,35 litres.
molar volume
The volume is 102 mL.
The volume is 22,1 L.
22.4 L. At STP 1 mole of any gas will always be equal to 22.4 L.
22.4 liters.
stupid question
This volume is 79,79 litres.
At STP, 1 mole of a gas will occupy 22.4 liters; or 0.5 mole will occupy 11.2 liters.
At STP, 1 mole of a gas will occupy 22.4 liters; or 0.5 mole will occupy 11.2 liters.
We know that one mole of any gas at STP occupies 22.4 liters of volume. We also know that one mole of carbon dioxide is 44.01 grams of CO2. If there are 44.01 grams of this gas in 22.4 liters at STP, then there will be about 0.98 grams of CO2 in half a liter (500 ml) of the gas at STP.