How many grams of water will be required to completely react with 1.00 mol of CaO according to the following reaction CaO+H2O__Ca(OH)2

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Verified Answer :

Hagrid Hagrid · Answer 1 · 2016-03-29T10:07:29-04:00

Given:

1.0
mol of CaO

Required:

grams of water

Solution:

CaO + H2O → Ca(OH)2

Molar mass of H2O = 18.02g H2O

1mol CaO(1 mol H2O/1 mol CaO)(18.02g H2O/1 mol H2O) = 0.055g H2O

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RomeliaThurston RomeliaThurston · Answer 2 · 2019-03-26T08:02:17-04:00

Answer: The mass of water required will be 18 grams.

Explanation:

For the given chemical reaction:

\(CaO+H_2O\rightarrow Ca(OH)_2\)

By Stoichiometry of the reaction:

1 mole of calcium oxide reacts with 1 mole of water.

So, 1 mole of calcium oxide will react with = \(\frac{1}{1}\times 1=1\) mole of water.

To calculate the mass of water required, we use the equation:

\(\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}\)

We are given:

Moles of water = 1 mole

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

\(1mol=\frac{\text{Mass of }H_2O}{18g/mol}\\\\\text{Mass of }H_2O=18g\)

Hence, the mass of water required will be 18 grams.