The value of `Delta H` for the combustion of C(s) is - 94.4 Kcal. The heat of formation of `CO_(2)(g)` is :-

Options

A. `-49.5` Kcal
B. `-94.4` K cal
C. `-188.0` K cal
D. More data required

Explanation

To find the heat of formation of carbon dioxide (CO₂), we can use the information provided about the combustion of carbon (C). The combustion reaction can be represented as follows:

1. **Write the combustion reaction**:
\[ C(s) + O_2(g) \rightarrow CO_2(g) \]

2. **Identify the given data**:
The enthalpy change (ΔH) for the combustion of carbon is given as:
\[ \Delta H = -94.4 \text{ kcal} \]

3. **Understand the concept of heat of formation**:
The heat of formation (ΔH_f) of a compound is defined as the change in enthalpy when one mole of the compound is formed from its elements in their standard states. In this case, the formation of CO₂ from carbon and oxygen is exactly what the combustion reaction describes.

4. **Relate the combustion reaction to the heat of formation**:
The ΔH for the combustion of carbon is equal to the heat of formation of CO₂ but with the opposite sign because the combustion reaction releases heat (exothermic). Therefore, the heat of formation of CO₂ can be expressed as:
\[ \Delta H_f (CO_2) = -\Delta H_{combustion} \]

5. **Calculate the heat of formation**:
Substituting the value of ΔH for combustion:
\[ \Delta H_f (CO_2) = -(-94.4 \text{ kcal}) = 94.4 \text{ kcal} \]

6. **Conclusion**:
The heat of formation of carbon dioxide (CO₂) is:
\[ \Delta H_f (CO_2) = 94.4 \text{ kcal} \]

### Final Answer:
The heat of formation of CO₂ is 94.4 kcal.

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