what mass of cu(io3)2 can be formed from 0.400 g of cuso4 5h2o
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mm = molar mass
0.400 g CuSO4.5H2O x (mm Cu(IO3)2/mm CuSO4.5H2O) = ?
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To determine the mass of Cu(IO3)2 that can be formed from 0.400 g of CuSO4 · 5H2O, you need to use stoichiometry and the molar masses of the compounds involved.
First, let's break down the given information:
- CuSO4 · 5H2O is the copper sulfate pentahydrate.
- Cu(IO3)2 is the copper(II) iodate compound.
Now, let's follow these steps to find the mass of Cu(IO3)2:
Step 1: Calculate the molar mass of CuSO4 · 5H2O.
CuSO4: Copper (Cu) has a molar mass of 63.55 g/mol. Sulfur (S) has a molar mass of 32.06 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol.
H2O: Hydrogen (H) has a molar mass of 1.01 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol.
Therefore, the molar mass of CuSO4 · 5H2O is:
(63.55 g/mol Cu + 32.06 g/mol S + (4 × 16.00 g/mol O)) + (5 × (2 × 1.01 g/mol H + 16.00 g/mol O))
Step 2: Calculate the molar mass of Cu(IO3)2.
Cu(IO3)2: Copper (Cu) has a molar mass of 63.55 g/mol, iodine (I) has a molar mass of 126.90 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol.
Therefore, the molar mass of Cu(IO3)2 is:
(63.55 g/mol Cu) + (2 × (126.90 g/mol I + 3 × 16.00 g/mol O))
Step 3: Calculate the moles of CuSO4 · 5H2O.
Divide the given mass of CuSO4 · 5H2O (0.400 g) by its molar mass, calculated in Step 1.
Step 4: Use stoichiometry to find moles of Cu(IO3)2.
The balanced chemical equation should allow us to relate the moles of CuSO4 · 5H2O to the moles of Cu(IO3)2. Unfortunately, it seems that the balanced equation is missing, which makes it impossible to determine the stoichiometry of the reaction.