Question

Each copper (II) sulfate unit is associated with five water molecules in crystalline copper (II) sulfate pentahydrate. When this compound is heated in air above 100 °C, it loses the water molecules and the blue color: CuSO4·5H2O → CuSO4 + 5H2O If 9.60 g of CuSO4 are left after heating 15.01 g of the blue compound, calculate the number of moles of water originally present in the compound.

Name: each copper ii sulfate unit is associated with five water molecules in crystalline copper ii sulfate pentahydrate when this compound is heated in air above 100 oc it loses the water molecule 13778
Uploaded: 2023-07-23T06:48:16-08:00
Duration: 1 min 13 s
Channel: Adi S
Description: each copper ii sulfate unit is associated with five water molecules in crystalline copper ii sulfate pentahydrate when this compound is heated in air above 100 oc it loses the water molecule 13778

          Each copper (II) sulfate unit is associated with five water molecules in crystalline copper (II) sulfate pentahydrate. When this compound is heated in air above 100 °C, it loses the water molecules and the blue color:
CuSO4·5H2O → CuSO4 + 5H2O
If 9.60 g of CuSO4 are left after heating 15.01 g of the blue compound, calculate the number of moles of water originally present in the compound.

Added by Miguel T.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

07/23/2023

Step 1

The molar mass of CuSO4 is approximately 159.61 g/mol. The molar mass of CuSO4·5H2O is approximately 249.68 g/mol. Show more…

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Each copper (II) sulfate unit is associated with five water molecules in crystalline copper (II) sulfate pentahydrate. When this compound is heated in air above 100 °C, it loses the water molecules and the blue color: CuSO4·5H2O → CuSO4 + 5H2O If 9.60 g of CuSO4 are left after heating 15.01 g of the blue compound, calculate the number of moles of water originally present in the compound.