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Answer :
If 85.0 grams of Ca(OH)₂ are used in the reaction, the mass in grams of water would be produced is 20.67 g.
The correct option is not given.
How many grams of water would be produced?
The mass of water produced is determined as follows:
Equation of reaction:
Ca(OH)₂ ---> CaO + H₂O
The mole ratio of the reaction shows that 1 mole of Ca(OH)₂ decomposes to yield 1 mole of CaO and 1 mole of H₂O.
Molar mass of Ca(OH)₂ = 74 g
Molar mass of H₂O = 18 g
74 g of Ca(OH)₂ decomposes to produce 18 g H₂O.
The mass of water produced from 85.0 grams of Ca(OH)₂ = 85 * 18/74
The mass of water produced from 85.0 grams of Ca(OH)₂ = 20.67 g
Learn more about mole ratio at: https://brainly.com/question/26023
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