This problem is providing us with the balanced chemical equation whereby cupper (II) nitrate is produced from copper and nitric acid. Thus, the produced grams of water are required and found to be 92.8 g as shown below:
In chemistry, stoichiometry is a tool for us to perform mole-mass relationships given a balanced chemical equation. In such a way, since this problem points out the moles of nitric acid that are consumed, one can write the following stoichiometric setup:
[tex]10.3molHNO_3*\frac{4molH_2O}{8molHNO_3} *\frac{18.02gH_2O}{1molH_2O}[/tex]
Where 4:8 is the mole ratio of water to nitric acid and 18.02 the molar mass of water. Hence, the result turns out to be:
[tex]92.8gH_2O[/tex]
Learn more about stoichiometry: https://brainly.com/question/9743981
