The heat evolved during the combination of 24 g C and 128 g S following the change is
`C+S_(2)rarrCS_(2),DeltaH=22.0 kcal`

Options

A. 11 kcal
B. 32 kcal
C. 44 kcal
D. 22 kcal

Explanation

To solve the problem, we need to determine the heat evolved during the reaction of 24 g of carbon (C) with 128 g of sulfur (S) to form carbon disulfide (CS₂). The given reaction has a standard enthalpy change (ΔH) of 22.0 kcal for the formation of CS₂ from C and S₂.

### Step-by-Step Solution:

1. **Determine the Molar Masses**:
- The molar mass of carbon (C) = 12 g/mol.
- The molar mass of sulfur (S) = 32 g/mol.

2. **Calculate the Moles of Reactants**:
- Moles of carbon (C):
\[ \text{Moles of C} = \frac{\text{mass of C}}{\text{molar mass of C}} = \frac{24 \text{ g}}{12 \text{ g/mol}} = 2 \text{ moles} \]
- Moles of sulfur (S):
\[ \text{Moles of S} = \frac{\text{mass of S}}{\text{molar mass of S}} = \frac{128 \text{ g}}{32 \text{ g/mol}} = 4 \text{ moles} \]

3. **Identify the Stoichiometry of the Reaction**:
- The balanced reaction is:
\[ C + 2S \rightarrow CS_2 \]
- From the balanced equation, 1 mole of C reacts with 2 moles of S to produce 1 mole of CS₂.

4. **Determine the Limiting Reactant**:
- For 2 moles of C, we need:
\[ 2 \text{ moles of C} \times 2 \text{ moles of S/mole of C} = 4 \text{ moles of S} \]
- Since we have exactly 4 moles of S, both reactants are present in the required stoichiometric ratio.

5. **Calculate the Heat Evolved**:
- The ΔH for the reaction is given as 22.0 kcal for the formation of 1 mole of CS₂.
- Since we are forming 2 moles of CS₂ (from 2 moles of C), the total heat evolved will be:
\[ \text{Heat evolved} = 2 \text{ moles of CS₂} \times 22.0 \text{ kcal/mole} = 44.0 \text{ kcal} \]

### Final Answer:
The heat evolved during the combination of 24 g of carbon and 128 g of sulfur is **44.0 kcal**.