What mass of water will be produced from 2.70 moles of Ca(OH)2 reacting with HCI

97.2g

Explanation:

Step 1:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

Ca(OH)2 + 2HCl —> CaCl2 + 2H2O

Step 2:

Determination of the number of mole of water (H2O) to produce from the reaction.

This is illustrated below:

From the balanced equation above,

1 mole of Ca(OH)2 produced 2 moles of H2O.

Therefore, 2.70moles of Ca(OH)2 will produce = 2.7 x 2 = 5.4 moles of H2O.

Step 3:

Converting 5.4 moles of H2O to grams. This is illustrated below:

Number of mole of H2O = 5.4 moles

Molar Mass of H2O = (2x1) + 16 = 2 + 16 = 18g/mol

Mass of H2O =?

Mass = number of mole x molar Mass

Mass of H2O = 5.4 x 18

Mass of H2O = 97.2g

Therefore, 97.2g of water is produced from the reaction.