2.750 g of copper(II) oxide, CuO2, was reduced by heating at high pressure with excess hydrogen to yield 2.196 g of copper Cu.
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To calculate the mass of copper(II) oxide, CuO2, initially present, we can subtract the mass of copper obtained from the mass of copper(II) oxide reduced.
Mass of copper(II) oxide, CuO2 = 2.750 g - 2.196 g
= 0.554 g
Therefore, the initial mass of copper(II) oxide, CuO2, present was 0.554 g.
To determine the mass of copper that was produced by the reduction of copper(II) oxide, we need to calculate the difference in mass before and after the reaction. Here's how you can do it:
1. Calculate the molar mass of CuO2:
- Copper (Cu) has an atomic mass of 63.55 g/mol.
- Oxygen (O) has an atomic mass of 16.00 g/mol.
- Since there are two oxygen atoms in CuO2, the molar mass of CuO2 is:
Cu = 63.55 g/mol + (2 * 16.00 g/mol) = 95.55 g/mol.
2. Calculate the number of moles of CuO2:
- Given that the mass of CuO2 is 2.750 g, we can determine the number of moles using the formula:
Moles = Mass / Molar mass.
Moles = 2.750 g / 95.55 g/mol ≈ 0.0287 mol.
3. Determine the stoichiometry of the reaction:
- From the chemical equation, we can see that for every mole of CuO2, one mole of Cu is produced:
CuO2 → 2Cu.
4. Calculate the number of moles of Cu produced:
- Since the stoichiometry of the reaction is 1:2 (CuO2:Cu), the moles of Cu produced will be twice the moles of CuO2 consumed:
Moles of Cu = 0.0287 mol * 2 = 0.0574 mol.
5. Calculate the mass of copper produced:
- Given the molar mass of copper is 63.55 g/mol, we can calculate the mass using:
Mass = Moles × Molar mass.
Mass = 0.0574 mol * 63.55 g/mol ≈ 2.896 g.
Therefore, the mass of copper produced by the reduction of copper(II) oxide is approximately 2.896 g.