Sure, let's calculate the mass for each of the given compounds.
### Part (a): Mass of 0.01 moles of Copper (II) Sulphate (CuSO₄)
1. Determine the molar mass of Copper (II) Sulphate (CuSO₄):
- The molar mass of Copper (Cu) is 64 g/mol.
- The molar mass of Sulfur (S) is 32 g/mol.
- The molar mass of Oxygen (O) is 16 g/mol.
The formula for Copper (II) Sulphate is CuSO₄, which has:
- 1 Copper (Cu) atom,
- 1 Sulfur (S) atom,
- 4 Oxygen (O) atoms.
Therefore, the molar mass of CuSO₄ can be calculated as:
[tex]\[
\text{Molar mass of CuSO₄} = (1 \times 64) + (1 \times 32) + (4 \times 16)
\][/tex]
Simplifying the calculation:
[tex]\[
\text{Molar mass of CuSO₄} = 64 + 32 + 64 = 160 \text{ g/mol}
\][/tex]
2. Calculate the mass of 0.01 moles of CuSO₄:
[tex]\[
\text{Mass} = \text{moles} \times \text{molar mass}
\][/tex]
Inserting the values:
[tex]\[
\text{Mass} = 0.01 \text{ moles} \times 160 \text{ g/mol} = 1.6 \text{ grams}
\][/tex]
So, the mass of 0.01 moles of CuSO₄ is 1.6 grams.
### Part (b): Mass of 0.5 moles of Lead (IV) Oxide (PbO₂)
1. Determine the molar mass of Lead (IV) Oxide (PbO₂):
- The molar mass of Lead (Pb) is 207 g/mol.
- The molar mass of Oxygen (O) is 16 g/mol.
The formula for Lead (IV) Oxide is PbO₂, which has:
- 1 Lead (Pb) atom,
- 2 Oxygen (O) atoms.
Therefore, the molar mass of PbO₂ can be calculated as:
[tex]\[
\text{Molar mass of PbO₂} = (1 \times 207) + (2 \times 16)
\][/tex]
Simplifying the calculation:
[tex]\[
\text{Molar mass of PbO₂} = 207 + 32 = 239 \text{ g/mol}
\][/tex]
2. Calculate the mass of 0.5 moles of PbO₂:
[tex]\[
\text{Mass} = \text{moles} \times \text{molar mass}
\][/tex]
Inserting the values:
[tex]\[
\text{Mass} = 0.5 \text{ moles} \times 239 \text{ g/mol} = 119.5 \text{ grams}
\][/tex]
So, the mass of 0.5 moles of PbO₂ is 119.5 grams.
### Summary:
- The mass of 0.01 moles of CuSO₄ is 1.6 grams.
- The mass of 0.5 moles of PbO₂ is 119.5 grams.
