Question

...Cr(OH)3(s)+...OH−=...CrO−2+...H2O...Cr(OH)3(s)+...OH−=...CrO2−+...H2O

When 1.00 mole of CrO−2CrO2− is formed , ___ grams of water will be produced.

• A. 9.0 grams
• B. 18.0 grams
• C. 27.0 grams
• D. 36.0 grams

Answer 1

The correct option is D 36.0 grams

The balanced chemical equation is
$Cr\left(OH{)}_3\right(s)+O{H}^{-}=Cr{O}_2^{-}+2H_{2}O$
When 1.00 mole of $Cr{O}_2^{-}$ is formed , 2 moles of water will be produced.
The molecular weight of water is 18 g/mol.
2 moles of water corresponds to $2\times 18=36$ g.
When 1.00 mole of $Cr{O}_2^{-}$ is formed , 36 grams of water will be produced.
Hence, option (D) is the correct answer.