How many moles of H2O are needed to react with 15.0g of CaO forming Ca (OH)2?
CaO + H2O --> Ca (OH)2
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To determine the number of moles of H2O needed to react with 15.0g of CaO, we need to use the balanced chemical equation and perform a stoichiometric calculation.
The first step is to write down the balanced chemical equation:
CaO + H2O -> Ca(OH)2
According to the equation, one mole of CaO reacts with one mole of H2O to produce one mole of Ca(OH)2.
Next, we need to calculate the molar mass of CaO:
CaO: 1 atom of calcium (40.08 g/mol) + 1 atom of oxygen (16.00 g/mol)
= 40.08 g/mol + 16.00 g/mol
= 56.08 g/mol
Now, we can use the molar mass of CaO and the given mass of 15.0g to calculate the number of moles of CaO:
moles of CaO = mass of CaO / molar mass of CaO
= 15.0g / 56.08 g/mol
= 0.267 mol
Since the balanced chemical equation tells us that one mole of CaO reacts with one mole of H2O, the number of moles of H2O needed is also 0.267 mol.
Therefore, 0.267 moles of H2O are needed to react with 15.0g of CaO, forming Ca(OH)2.