Each copper(II) sulfate unit is associated with five water molecules in crystalline copper(II) sulfate pentahydrate (CuSO 4 .·5 H2 O) ·When this compound is heated in air above 100^∘ C, it loses the water molecules and also its blue color: CuSO4 ·5 H2 O ⟶CuSO4 5 H2 O If 9.60 g of CuSO4 are left after heating 15.01 g of the blue compound, calculate the number of moles of H2 O originally present in the compound. | Numerade
Each copper(II) sulfate unit is associated with five water molecules in crystalline copper(II) sulfate pentahydrate (CuSO 4 .·5 H2 O) ·When this compound is heated in air
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SOLVED: Calcium sulfate, CaSO4, is a white, crystalline powder. Gypsum is a mineral, or natural substance, that is a hydrate of calcium sulfate. A 100 g sample of gypsum contains 0.791 g CaSO4. How many moles of CaSO4 are there in this sample? Assuming that the rest of the sample is water, how many moles of H2O are there in the sample? How is the result consistent with the formula CaSO4 · 2H2O? Calculate the following:- Number of atoms in 8.21 g Li- Number of atoms in 32.0 g Br2- Number of mole
SOLVED: Calcium sulfate, CaSO4, is a white, crystalline powder. Gypsum is a mineral, or natural substance, that is a hydrate of calcium sulfate. A 100 g sample of gypsum contains 0.791 g CaSO4. How many moles of CaSO4 are there in this sample? Assuming that the rest of the sample is water, how many moles of H2O are there in the sample? How is the result consistent with the formula CaSO4 · 2H2O? Calculate the following:- Number of atoms in 8.21 g Li- Number of atoms in 32.0 g Br2- Number of mole
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