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Answer: Each copper(II) sulfate unit is associated with
Chapter 3, Problem 73P(choose chapter or problem)
Each copper(II) sulfate unit is associated with five water molecules in crystalline copper(II) sulfate pentahydrate \(\left(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\right)\). When this compound is heated in air above \(100^{\circ} \mathrm{C}\), it loses the water molecules and also its blue color:
\(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{CuSO}_{4}+5 \mathrm{H}_{2} \mathrm{O}\)
If 9.60 g of \(\mathrm{CuSO}_{4}\) are left after heating 15.01 g of the blue compound, calculate the number of moles of \(\mathrm{H}_{2} \mathrm{O}\) originally present in the compound.
Questions & Answers
QUESTION:
Each copper(II) sulfate unit is associated with five water molecules in crystalline copper(II) sulfate pentahydrate \(\left(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\right)\). When this compound is heated in air above \(100^{\circ} \mathrm{C}\), it loses the water molecules and also its blue color:
\(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{CuSO}_{4}+5 \mathrm{H}_{2} \mathrm{O}\)
If 9.60 g of \(\mathrm{CuSO}_{4}\) are left after heating 15.01 g of the blue compound, calculate the number of moles of \(\mathrm{H}_{2} \mathrm{O}\) originally present in the compound.
ANSWER:Step 1 of 2
Here we have to calculate the number of moles of 
The reaction is,
