15.3 litres of water will be produced if we take 1.7 litres of Hydrogen
Explanation:
Let's take a look over synthesis reaction;
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<u>Balancing the chemical reaction;</u>
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Thus, 2 moles of hydrogen molecules are required to form 2 moles of water molecules.
<u>Equating the molarity;</u>
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= ![\frac{x*1}{2*18}](https://tex.z-dn.net/?f=%5Cfrac%7Bx%2A1%7D%7B2%2A18%7D)
(Since, the molecular mass of hyd and water is 2 and 18 respectively)
x=![\frac{1.7*2*18}{2*2}](https://tex.z-dn.net/?f=%5Cfrac%7B1.7%2A2%2A18%7D%7B2%2A2%7D)
x= 15.3 litres.
Thus,15.3 L of water will be produced if we take 1.7 litres of Hydrogen in a synthesis reaction.
In the reactants Sb has oxidatin number 0 (because it is in its elemental form)
In the products Sb has oxidaton number +3.
Then Sb lost electrons which means it oxidized.
<span> F = ma = 40kg * 10m/s^2 = 400 kg-m/s^2 = 400N</span>
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