how much energy to separate hydrogen from oxygen?
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That means that 1 kilowatt hour of electricity can split about 270 grams of water and produce about 350 liters of hydrogen and 175 liters of oxygen. It depends on the pressures and concentrations. Assuming standard conditions (1 atmosphere of pressure, 1 mole per liter of H+ ions), then you'd need a voltage of 1.23V.
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Atomic and Molecular Weights Thus, oxygen was assigned an atomic mass of 16. We now know that a hydrogen atom has a mass of 1.6735 x 10-24 grams, and that the oxygen atom has a mass of 2.6561 X 10-23 grams.
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Compare your answer with the ionization energy fo H-atom (energy required to remove the electron from n= orbit ). Thus , 0.544eV energy is required to ionise H-atom of electron is in 5th orbit .
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The weight of unreacted H2=70 gm. The reaction is 2H2 + O2 gives 2H2O. That is one mole O2 requires two moles of hydrogen. And one mol H2 requirs half moles of O2. We have 80/2=40 mol H2 and 80/32=2.5 moles O2.
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For H2O, there is one atom of oxygen and two atoms of hydrogen. A molecule can be made of only one type of atom. In its stable molecular form, oxygen exists as two atoms and is written O2. to distinguish it from an atom of oxygen O, or ozone, a molecule of three oxygen atoms, O3.
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Oxygen (O2) produces less water (H2O) than hydrogen (H2) therefore oxygen is the limiting reactant.
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Until recently, the platinum catalyst that splits the hydrogen into an ion and an electron has been prohibitively expensive. Up to a few years ago, hydrogen fuel cells cost around $1000 for every kilowatt of power they generated – or around $100,000 per car.
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A. How much energy is required to break the first O–O bond? 349 kJ/mol is required to break the first O2 bond.
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Just breaking the hydrogen bond in liquid water, leaving the molecules essentially in the same position, requires only about 25% of this energy. This has been estimated at 6.3 kJ ˣ mol-1 [690], and only just over twice the average collision energy.
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1 kg of hydrogen contains 33.33 kWh of usable energy, whereas petrol and diesel only hold about 12 kWh/kg (see www.h2data.de). In terms of volumetric energy density however, hydrogen is outperformed by liquid fuels.
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Expert Answers info 1 mole of water requires 1 mole of hydrogen (H2) and 0.5 moles of oxygen (O2). This requires 100/18 moles of hydrogen. As the molar mass of hydrogen is 2, it requires 200/18 = 100/9 g of hydrogen. It requires 100/9 g of hydrogen gas and 800/9 g of oxygen gas to make 100 g of water.
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For example, to find the ratio of mass of hydrogen to oxygen in water, divide the total molar mass of hydrogen, 2.016, by the molar mass of oxygen, 16.00 and get 0.126. To find the ratio of oxygen to hydrogen, divide 16.00 by 2.016 and get 7.937.
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The mass (m) of hydrogen is: [ m=5.357142857×2.0 ] = 10.7 grams. Note that: this answer is rounded to 3 significant figures. Therefore, 10.7 grams of Hydrogen are necessary to fully react with 50.0 grams of Nitrogen.
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The simplest method to obtain hydrogen by electrolysis is the hydrolysis of water. This method can be used to obtain pure oxygen and hydrogen in the laboratory.
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For H2O, there is one atom of oxygen and two atoms of hydrogen. A molecule can be made of only one type of atom.
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Theoretically, a ratio of 2:1 hydrogen:oxygen is enough to achieve maximum efficiency; in practice a ratio 4:1 or 5:1 is needed to avoid an oxidizing flame.
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Depending on the nature of the donor and acceptor atoms which constitute the bond, their geometry, and environment, the energy of a hydrogen bond can vary between 1 and 40 kcal/mol. This makes them somewhat stronger than a van der Waals interaction, and weaker than fully covalent or ionic bonds.