Final answer:
To find the mass of Cu(NO₃)₂ that can be prepared, we calculate the moles of copper and nitric acid and compare the mole ratios to determine the limiting reactant. Then, we use the limiting reactant's moles to calculate the mass of Cu(NO₃)₂.
Step-by-step explanation:
To calculate the mass of Cu(NO₃)₂ that can be prepared from the given reaction, we need to determine the limiting reactant.
First, calculate the moles of copper and HNO₃ using their molar masses:
Moles of Cu = 3.65 g / 63.55 g/mol = 0.0575 mol
Moles of HNO₃ = 5.16 g / 63.01 g/mol = 0.0819 mol
Next, compare the mole ratios of Cu(NO₃)₂ to Cu and HNO₃:
From the balanced equation, the mole ratio of Cu(NO₃)₂ to Cu is 3:1, and the mole ratio of Cu(NO₃)₂ to HNO₃ is 2:8.
Since the mole ratio of Cu(NO₃)₂ to HNO₃ is 2:8, we compare the moles of HNO₃ to determine the limiting reactant:
0.0819 mol HNO₃ * (2/8) = 0.0205 mol Cu(NO₃)₂ (limiting reactant)
Finally, calculate the mass of Cu(NO₃)₂ that can be prepared:
Mass of Cu(NO₃)₂ = moles of Cu(NO₃)₂ * molar mass of Cu(NO₃)₂
= 0.0205 mol * 187.57 g/mol = 3.85 g