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This volume is 79,79 litres.
0.25 moles
Ideal gas equation. PV = nRT ===============
I mole - 16g of methane is 1 mole. At STP it would occupy 22.4 liters
The volume is approx. 15,35 litres.
This volume is 79,79 litres.
0.25 moles
Ideal gas equation. PV = nRT ===============
I mole - 16g of methane is 1 mole. At STP it would occupy 22.4 liters
The volume is approx. 15,35 litres.
At standard temperature and pressure, 1 mole of any gas will occupy 22.4 liters. Set up a direct proportion of 22.4 liters/1 mole = 1 liter/x moles and solve for x. You get 0.045 moles.
1 mole occupies 22.4 liters. 0.5 moles occupies 11.2 liters at STP.
How many molecules are in 30 liters of methane (CH4) at STP
1 mole occupies 22.414 liters So, 3.30 moles will occupy 73.966 liters.
8,4 liters of nitrous oxide at STP contain 2,65 moles.
16,8 L of Xe gas at STP is equivalent to 0,754 moles.
The easiest way to approach this is to remember molar volume: one mole of every (ideal) gas will occupy 22.4 liters at STP - a gas occupies 22.4 L/mol. Since we know that, we can set up a simple proportion that follows the thought process: if one mole of a gas occupies 22.4 liters (at STP), then 2.88 grams of methane occupies x liters. But before we do that, we have a problem: the measurement given is in the wrong units - it is in grams when molar volume is in moles. Therefore, we first need to convert 2.88 grams of methane to moles. To do this, we need the molar mass of the compound - the sum of all the atomic masses involved. Carbon = 12.0 grams Hydrogen = 1.01 grams × 4 atoms = 4.04 grams ------------------------------------------------------------- Methane = 16.04 grams To convert grams to moles: Grams of substance ÷ Molar mass (in grams) = Moles of substance 2.88 grams CH4 ÷ 16.04 grams CH4 = 0.180 moles CH4 Now we follow through with our proportion: 22.4 L/1 mol = x L/.180 mol x = 4.03 L 2.88 grams of methane occupies 4.03 liters at STP