How many of g of S are required to produce 10 moles and 30 g of `H_(2)SO_(4)` respectively?

Options

A. 320g,9.79g
B. 640g,9.79g
C. 9.79g,640g
D. 9.79g,320g

Explanation

To solve the problem of how many grams of sulfur (S) are required to produce 10 moles and 30 grams of H₂SO₄, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Composition of H₂SO₄**:
- The chemical formula for sulfuric acid (H₂SO₄) indicates that each molecule contains one atom of sulfur (S).
- The molar mass of H₂SO₄ is calculated as follows:
- Hydrogen (H): 1 g/mol × 2 = 2 g/mol
- Sulfur (S): 32 g/mol × 1 = 32 g/mol
- Oxygen (O): 16 g/mol × 4 = 64 g/mol
- Total molar mass of H₂SO₄ = 2 + 32 + 64 = 98 g/mol

2. **Calculating Sulfur for 10 Moles of H₂SO₄**:
- Since 1 mole of H₂SO₄ contains 32 grams of sulfur, for 10 moles:
\[ \text{Grams of S} = 10 \, \text{moles} \times 32 \, \text{g/mol} = 320 \, \text{grams} \]

3. **Calculating Sulfur for 30 Grams of H₂SO₄**:
- First, we need to find out how many moles are in 30 grams of H₂SO₄:
\[ \text{Moles of H₂SO₄} = \frac{\text{mass}}{\text{molar mass}} = \frac{30 \, \text{g}}{98 \, \text{g/mol}} \approx 0.306 \, \text{moles} \]
- Now, calculate the grams of sulfur in 30 grams of H₂SO₄:
\[ \text{Grams of S} = 0.306 \, \text{moles} \times 32 \, \text{g/mol} \approx 9.79 \, \text{grams} \]

### Final Results:
- To produce **10 moles of H₂SO₄**, **320 grams** of sulfur are required.
- To produce **30 grams of H₂SO₄**, approximately **9.79 grams** of sulfur are required.