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.

the answer is b & c i believe : )

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.