Question
calculating the volume of H2SO4 required to produce a given amount of H2 gas
Answers
Answered by
GPT-4o mini
To calculate the volume of sulfuric acid (H₂SO₄) required to produce a specific amount of hydrogen gas (H₂), we need to consider the chemical reaction involved.
The reaction of sulfuric acid with a metal, such as zinc (Zn), is a common way to produce hydrogen gas:
\[
\text{Zn} + \text{H₂SO₄} \rightarrow \text{ZnSO₄} + \text{H₂}
\]
From the balanced equation, we can see that 1 mole of zinc reacts with 1 mole of sulfuric acid to produce 1 mole of hydrogen gas.
### Steps to Calculate Volume of H₂SO₄ Required
1. **Determine Moles of H₂ Required**:
Use the ideal gas law, where at standard temperature and pressure (STP: 0°C and 1 atm), 1 mole of an ideal gas occupies 22.4 liters.
If you know the desired volume of H₂ gas, you can calculate moles of H₂:
\[
\text{Moles of H₂} = \frac{\text{Volume of H₂ (in liters)}}{22.4 \, \text{L/mol}}
\]
2. **Relate Moles of H₂ to Moles of H₂SO₄**:
Since 1 mole of H₂SO₄ produces 1 mole of H₂, the moles of H₂SO₄ needed will be equal to the moles of H₂ calculated in the previous step.
3. **Calculate the Volume of H₂SO₄**:
The concentration of sulfuric acid is usually needed to determine the volume. If you know the concentration (C) of the H₂SO₄ solution (in mol/L), you can find the volume (V) using the formula:
\[
\text{Volume of H₂SO₄ (L)} = \frac{\text{Moles of H₂SO₄}}{C}
\]
### Example Calculation
Let's say you want to produce 11.2 liters of H₂ gas at STP.
1. Calculate moles of H₂:
\[
\text{Moles of H₂} = \frac{11.2 \, L}{22.4 \, L/mol} = 0.5 \, \text{moles}
\]
2. Moles of H₂SO₄ required:
\[
\text{Moles of H₂SO₄} = 0.5 \, \text{moles}
\]
3. If you have a 1 M solution of H₂SO₄ (1 mole/L):
\[
\text{Volume of H₂SO₄} = \frac{0.5 \, \text{moles}}{1 \, \text{mol/L}} = 0.5 \, \text{L} \text{ or } 500 \, \text{mL}
\]
This means you would need 500 mL of 1 M H₂SO₄ to generate 11.2 liters of H₂ gas at STP. Adjust the calculations based on the actual concentration of your H₂SO₄ solution.
The reaction of sulfuric acid with a metal, such as zinc (Zn), is a common way to produce hydrogen gas:
\[
\text{Zn} + \text{H₂SO₄} \rightarrow \text{ZnSO₄} + \text{H₂}
\]
From the balanced equation, we can see that 1 mole of zinc reacts with 1 mole of sulfuric acid to produce 1 mole of hydrogen gas.
### Steps to Calculate Volume of H₂SO₄ Required
1. **Determine Moles of H₂ Required**:
Use the ideal gas law, where at standard temperature and pressure (STP: 0°C and 1 atm), 1 mole of an ideal gas occupies 22.4 liters.
If you know the desired volume of H₂ gas, you can calculate moles of H₂:
\[
\text{Moles of H₂} = \frac{\text{Volume of H₂ (in liters)}}{22.4 \, \text{L/mol}}
\]
2. **Relate Moles of H₂ to Moles of H₂SO₄**:
Since 1 mole of H₂SO₄ produces 1 mole of H₂, the moles of H₂SO₄ needed will be equal to the moles of H₂ calculated in the previous step.
3. **Calculate the Volume of H₂SO₄**:
The concentration of sulfuric acid is usually needed to determine the volume. If you know the concentration (C) of the H₂SO₄ solution (in mol/L), you can find the volume (V) using the formula:
\[
\text{Volume of H₂SO₄ (L)} = \frac{\text{Moles of H₂SO₄}}{C}
\]
### Example Calculation
Let's say you want to produce 11.2 liters of H₂ gas at STP.
1. Calculate moles of H₂:
\[
\text{Moles of H₂} = \frac{11.2 \, L}{22.4 \, L/mol} = 0.5 \, \text{moles}
\]
2. Moles of H₂SO₄ required:
\[
\text{Moles of H₂SO₄} = 0.5 \, \text{moles}
\]
3. If you have a 1 M solution of H₂SO₄ (1 mole/L):
\[
\text{Volume of H₂SO₄} = \frac{0.5 \, \text{moles}}{1 \, \text{mol/L}} = 0.5 \, \text{L} \text{ or } 500 \, \text{mL}
\]
This means you would need 500 mL of 1 M H₂SO₄ to generate 11.2 liters of H₂ gas at STP. Adjust the calculations based on the actual concentration of your H₂SO₄ solution.