Answer:
Water has a molar mass of 18.015 g/mol . This means that one mole of water molecules has a mass of 18.015 g . So, to sum this up, 6.022⋅1023 molecules of water will amount to 1 mole of water, which in turn will have a mass of 18.015 g . 2.7144moles H2O ⋅6.022⋅1023molec.
Explanation:
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Answer is: 10 moles of water will be produced.
Balanced chemical reaction of formation of water:
2H₂ + O₂ → 2H₂O.
n(H₂) = 10 mol; amount of hydrogen gas.
From balanced chemical reaction: n(H₂) : n(H₂O) = 2 : 2 (1 : 1).
n(H₂O) = n(H₂).
n(H₂O) = 10 mol; amount of water.
Electrons fill the electron orbitals (s, p, d, or f) starting from the lowest energy level going to the highest energy level.
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The quantity of heat required to vapourize 1 mole of a substance depends on the kind of intermolecular forces between the molecules of the substance. Diethyl ether molecules are held together by weak dispersion forces compared to the stronger hydrogen bonding in ethanol. Therefore, 1 mole of diethyl ether requires less heat to vapourize than is required to vapourize 1 mole of ethanol.
Intermolecular forces hold the molecules a substance together in a given state of matter. The properties of a substance such as boiling point, melting point etc are dependent on the nature of intermolecular forces holding the molecules of the substance.
Diethyl ether molecules are held together by weak dispersion forces while molecules of ethanol are held together by hydrogen bonds.
Since hydrogen bonds are much stronger than dispersion forces, a greater quantity of heat is required to break the intermolecular hydrogen bonds in ethanol in order to vapourize them than is required to vapourize diethyl ether.
Therefore, owing to stronger intermolecular forces between molecules of ethanol, less heat is required to vapourize than is required to vapourize 1 mole of ethanol.
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