Question
. How many moles of aluminum sulfate would
you have? How many molecules of aluminum sulfate would be present?
you have? How many molecules of aluminum sulfate would be present?
Answers
GPT-4o mini
To calculate the number of moles of aluminum sulfate (Al₂(SO₄)₃), as well as the number of molecules, we need to know the mass of aluminum sulfate you have. If you could provide that information, I can help you with the calculations.
However, I can describe the general process:
1. **Calculate Moles**:
\[
\text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}
\]
The molar mass of aluminum sulfate can be calculated as follows:
- Aluminum (Al): 26.98 g/mol
- Sulfate (SO₄): 32.07 g/mol + 4 × 16.00 g/mol = 96.07 g/mol
- Therefore, the molar mass of Al₂(SO₄)₃:
\[
(2 \times 26.98) + (3 \times 96.07) = 53.96 + 288.21 = 342.17 \text{ g/mol}
\]
2. **Calculate Number of Molecules**:
The number of molecules can be calculated using Avogadro's number (\(6.022 \times 10^{23} \text{ molecules/mol}\)):
\[
\text{molecules} = \text{moles} \times 6.022 \times 10^{23} \text{ molecules/mol}
\]
If you provide the mass of aluminum sulfate you have, I can compute the specific values for you!
However, I can describe the general process:
1. **Calculate Moles**:
\[
\text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}
\]
The molar mass of aluminum sulfate can be calculated as follows:
- Aluminum (Al): 26.98 g/mol
- Sulfate (SO₄): 32.07 g/mol + 4 × 16.00 g/mol = 96.07 g/mol
- Therefore, the molar mass of Al₂(SO₄)₃:
\[
(2 \times 26.98) + (3 \times 96.07) = 53.96 + 288.21 = 342.17 \text{ g/mol}
\]
2. **Calculate Number of Molecules**:
The number of molecules can be calculated using Avogadro's number (\(6.022 \times 10^{23} \text{ molecules/mol}\)):
\[
\text{molecules} = \text{moles} \times 6.022 \times 10^{23} \text{ molecules/mol}
\]
If you provide the mass of aluminum sulfate you have, I can compute the specific values for you!