Question

According to the following reaction, how many grams of water are produced in the complete reaction of 31.8 grams of barium hydroxide?

Ba(OH)2(aq) + H2SO4(aq) --> BaSO4(s) + 2H2O(l)

Answer 1

6.696 g of water (H₂O)

Step-by-step explanation:

First we calculate the number of moles of barium hydroxide:

number of moles = mass / molecular weight

number of moles = 31.8 / 171.3 = 0.186 moles of barium hydroxide

Form the chemical reaction we may devise the following reasoning:

if 1 mole of barium hydroxide produces 2 moles of water

then 0.186 moles of barium hydroxide produces X moles of water

X = (0.186 × 2) / 1 = 0.372 moles of water

mass = number of moles × molecular weight

mass of water = 0.372 × 18 = 6.696 g