how much energy is required to extract hydrogen from water?
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Electrolysis of water However, current best processes for water electrolysis have an effective electrical efficiency of 70-80%, so that producing 1 kg of hydrogen (which has a specific energy of 143 MJ/kg or about 40 kWh/kg) requires 50–55 kWh of electricity.
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Combining all the energy input totals, Gleick and Cooley found that producing bottled water requires between 5.6 and 10.2 million joules of energy per liter, depending on transportation factors (a typical personal-sized water bottle is about 0.5 liters).
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… energy known as the latent heat of vaporization is required to break the hydrogen bonds. At 100 °C, 540 calories per gram of water are needed to convert one gram of liquid water to one gram of water vapour under normal pressure.
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Water is made up of two hydrogen (H) atoms and one oxygen (O) atom. The formula for water is H2O. The hydrogen atoms have filled orbitals with two electrons and the oxygen atom is filled with eight electrons.
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There are two hydrogen atoms per water molecule. There are 6.022x10^23 water molecules per mole. To calculate for 5 moles, (2 H atom)/(H2O molecule) X (6.022x10^23 H2O molecules)/(mole) X 5 moles = 6.022x10^24.
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The answer is 116 kJ . c - water's specific heat - 4.184 J/g⋅∘C . Then, you must provide enough heat to get all the water from liquid to steam. This is calculated using water's enthalpy of vaporization, ΔHvap - 40.68 kJ/mol .
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1 liter of water has a mass of 1 kg. If the water starts off at 100 degrees C, then the energy required to evaporate it would be 540,000 calories or 2.3 x 10^6 Joules. If the water begins at a temperature T degrees, then an additional (100 - T) x 10^3 calories would be required to raise its temperature to 100 degrees.
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An alternative method exists when water is electrolyzed to make oxygen and hydrogen that contains normal gas, along with deuterium. The hydrogen is then liquefied and distilled to separate the two components, then the deuterium is reacted with oxygen to form heavy water.
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Water is H2O so 5 Moles of water contains; 2 x 5 x 6.022140857 × 10^23 atoms of Hydrogen ! There are two hydrogen atoms per water molecule. There are 6.022x10^23 water molecules per mole.
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Art Connections. [link] The hydrolysis of one ATP molecule releases 7.3 kcal/mol of energy (∆G = −7.3 kcal/mol of energy).
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To convert 100.0 g of water at 20.0 °C to steam at 100.0 °C requires 259.5 kJ of energy.
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Energy is always required to break a bond, which is known as bond energy. The electrolysis of water requires a minimum of 237.13 kJ of electrical energy input to dissociate each mole. Each mole of water gives you 2 grams of Hydrogen and 16 grams of Oxygen.
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Water has a molar mass of 18.01528 g/mol≈18 g/mol . Since water has a chemical formula of H2O , there will be 2 moles of hydrogen in every mole of water. In one mole of water, there will exist approximately 6.02⋅1023 water molecules. So, there will be a total of 6.02⋅1023⋅2≈1.2⋅1024 hydrogen atoms.
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Two water molecules contain 4 hydrogen atoms and 2 oxygen atoms.
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Considering the industrial production of hydrogen, and using current best processes for water electrolysis (PEM or alkaline electrolysis) which have an effective electrical efficiency of 70–80%, producing 1 kg of hydrogen (which has a specific energy of 143 MJ/kg) requires 50–55 kW⋅h (180–200 MJ) of electricity.
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Notice that the reaction requires 2 moles of hydrogen gas and 1 mole of oxygen gas to produce 2 moles of water.
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1 liter of water has a mass of 1 kg. If the water starts off at 100 degrees C, then the energy required to evaporate it would be 540,000 calories or 2.3 x 10^6 Joules.