how many moles of water are there in 1 l at stp?
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Around 56 moles of water are there in 1.000 l at STP. It has been found that a single mole of a compound has a mass in grams equal to the molecular...
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1 Answer. In 78.41 liters of neon gas at STP, you have 3.498 moles of the gas.
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At STP 1 mole of an ideal gas = 22.4 liters. Assuming that water vapor behaves as an ideal gas, then... 0.08929 moles H2O x 6.02x1023 molecules/mol = 5.4x1022 molecules = 5x1022 molecules (1 sig. fig.)
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Therefore, 4 moles of water will have 4(6.022x10^23) number of water molecules.
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The question should have been how many molecules of oxygen are present in 1 litre of air containing 80% of O2. 1 mole of any gas at STp, occupies 22.4 litre. 22400ml of O2 gas contains 6.022x 10^23 molecules. =2.15 x 10^22 molecules.
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If you have 6.022⋅1023 molecules of water, then you can say for a fact that you have 1 mole of water. Now, you know that your sample contains 4.0 moles of water. In order to find the number of molecules of water it contains, you can use Avogadro's constant as a conversion factor.
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1 mole of any gas at STp, occupies 22.4 litre. 22400ml of O2 gas contains 6.022x 10^23 molecules. =2.15 x 10^22 molecules.
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The liter of water has 1000 grams. The number of moles is 1000/18 = 55.556 moles. The number of molecules is therefore 6.022*1023 * 55.556 = 3.346*1025 molecules.
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We find moles of water. All you have to do is just divide 75 by 18 and you'll get 4.17 moles of H2O.
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Conversions Between Moles and Gas Volume Molar volume at STP can be used to convert from moles to volume and from volume to moles for gaseous samples. The fact that 1 mole = 22.4 L is the basis for the conversion factor.
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The most common example is the molar volume of a gas at STP (Standard Temperature and Pressure), which is equal to 22.4 L for 1 mole of any ideal gas at a temperature equal to 273.15 K and a pressure equal to 1.00 atm.
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1 molecule of H2O contains 10electrons. So one mole that is equal to 22.4 L of H2O will contain 6.022 ×10^23 × 10 electrons. So 1.8 ml will have - 6.022×10^23×1.8×10/22.4 ×1000=6.022×10^21×1.8/22.4.
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At NTP 22.4 litres of a gas forms one mole that is 6.023×10^23 molecules. Volume of CO2 in 1 litre air= (0.03÷100)×1 litres.
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Because the reaction occurs at STP, 1 mole of NH3 gas occupies 22.4 L.
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If you have a compound like H2O, then: one mole of water contains 6.02 x 1023 MOLECULES of water. But each molecule of water contains 2 H and 1 O atom = 3 atoms, so there are approximately 1.8 x 1024 atoms in a mole of water.
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Since we have 4 moles of oxygen, we can put that directly into the equation. Assuming that oxygen is our limiting reactant (because it is not otherwise specified), we can find that per one mole of oxygen, we get two moles of water. This means that per four moles of oxygen, we get eight moles of water.
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Thus, for example, one mole of water contains 6.02214076×1023 molecules, whose total mass is about 18.015 grams – and the mean mass of one molecule of water is about 18.015 daltons.