Question

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

Answer 1

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

Answer 2

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

Step-by-step 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 =
`(1)/(1)* 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.