How many grams of water are theoretically produced for the following reaction given we have 2.6 moles of hcl and 1.4 moles of ca(oh)₂? reaction:

46.8 g of water are produced in the reaction

Explanation:

The reaction is:

2HCl + Ca(OH)₂  → 2H₂O + CaCl₂

We have the moles of each reactant, so let's determine the limiting reagent.

Ratio is 2:1 and 1:2

2 moles of acid need 1 mol of hydroxide to react.

2.6 moles of acid would need (2.6 .1)/2 = 1.3 moles

I have 1.4 moles of Ca(OH)₂, so this is the excess. Therefore the limiting reactant is the acid. Let's verify it.

1 mol of hydroxide needs 2 moles of acid, to react.

1.4 moles of Ca(OH) would need, the double. Of course, 1.4  .2 = 2.8 moles.

I only have 2.6 moles of acid, and is not enough.

As we found out the limiting reactant, we can work with the equation.

2 moles of HCl produce 2 moles of water. Ratio is 1:1

Therefore 2.6 moles of HCl will produce 2.6 moles of H₂O

When we convert the moles to mass, we obtain:

2.6 mol . 18 g/mol = 46.8 g

answer; the numbers of valence electrons in the acetic acid molecule (ch3co2h) is 24;