In carbon disulphide (`CS_2`), the mass of sulphur in combination with 3.0 g of carbon is:

Options

A. 4.0 g
B. 6.0 g
C. 64.0 g
D. 16.0 g

Explanation

To find the mass of sulfur in combination with 3.0 g of carbon in carbon disulfide (CS₂), we will follow these steps:

### Step 1: Determine the molar masses of carbon and sulfur.
- The molar mass of carbon (C) is 12 g/mol.
- The molar mass of sulfur (S) is 32 g/mol.

### Step 2: Write the chemical formula for carbon disulfide.
- The chemical formula for carbon disulfide is CS₂, which indicates that one atom of carbon combines with two atoms of sulfur.

### Step 3: Calculate the total mass of sulfur that combines with carbon.
- In CS₂, 1 mole of carbon (12 g) combines with 2 moles of sulfur (2 × 32 g = 64 g).
- Therefore, the ratio of the mass of sulfur to the mass of carbon in CS₂ is:
\[ \text{Mass of S} : \text{Mass of C} = 64 \text{ g} : 12 \text{ g} \]

### Step 4: Set up a proportion to find the mass of sulfur that combines with 3.0 g of carbon.
- Let \( x \) be the mass of sulfur that combines with 3.0 g of carbon. We can set up the proportion:
\[ \frac{64 \text{ g}}{12 \text{ g}} = \frac{x \text{ g}}{3.0 \text{ g}} \]

### Step 5: Solve for \( x \).
- Cross-multiply to solve for \( x \):
\[ 64 \text{ g} \times 3.0 \text{ g} = 12 \text{ g} \times x \]
\[ 192 = 12x \]
\[ x = \frac{192}{12} = 16 \text{ g} \]

### Conclusion:
- The mass of sulfur that combines with 3.0 g of carbon in carbon disulfide is **16 g**.

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