The observation that ethanol (C2H5OH) has a higher vapor pressure than water (H2O) at the same temperature is due to more
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Considering the reaction stoichiometry, the quantity of moles of H₂O produced is 3.02 moles.
The balanced reaction is:
CuO + H₂ → Cu + H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- CuO= 1 mole
- H₂= 1 mole
- Cu= 1 mole
- H₂O= 1 mole
The molar mass of the compounds present in the reaction is:
- CuO= 79.55 g/mole
- H₂= 2 g/mole
- Cu= 63.55 g/mole
- H₂O: 18 g/mole
Then, by reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of mass of each compound participate in the reaction:
- CuO= 1 mole× 79.55 g/mole= 79.55 grams
- H₂= 1 mole× 2 g/mole= 2 grams
- Cu= 1 mole× 63.55 g/mole= 63.55 grams
- H₂O: 1 mole× 18 g/mole= 18 grams
Then, it is possible to determine the moles of H₂O necessary by the following rule of three: If by reaction stoichiometry 79.55 grams of CuO produces 1 mole of H₂O, 240 grams of CuO produces how many moles of H₂O?
<u><em>moles of H₂O= 3.02 moles</em></u>
Finally, the quantity of moles of H₂O produced is 3.02 moles.
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