Answer:
BaCl₂·(H₂O)₂
Explanation:
The reaction that takes place is:
- BaCl₂·(H₂O)ₙ → BaCl₂ + nH₂O
The information given by the problem tells us that 5.00 g of reactant were consumed. Of those 5.00 g, 4.26 g were converted into BaCl₂, this means that the other 0.74 g were converted into water.
We convert 0.74 g of water into moles, using its molar mass:
- 0.74 g H₂O ÷ 18 g/mol = 0.041 mol H₂O
Then we convert 4.26 g of BaCl₂ into moles:
- 4.26 g BaCl₂ ÷ 208.23 g/mol = 0.0204 mol BaCl₂
We can write these results as (BaCl₂)₀.₀₂·(H₂O)₀.₀₄. We multiply those coefficients by 50 in order to make them integers, and we're left with:
