Smelting of iron ore takes place through this reaction
`2Fe_(2)O_(3)(s)+3C(s)rarr4Fe(s)+3CO_(2)(g)`
`DeltaH_(f)^(0)` of `Fe_(2)O_(3)` and `CO_(2)` are `-8242KJmol^(-1)` and `-393.7KJmol^(-1)`
The reaction is

Options

A. endothermic
B. exothermic
C. `DeltaH=0`
D. none of these

Explanation

To determine whether the smelting of iron ore is an endothermic or exothermic reaction, we need to calculate the enthalpy change (ΔH) for the reaction given:

\[ 2Fe_{2}O_{3}(s) + 3C(s) \rightarrow 4Fe(s) + 3CO_{2}(g) \]

### Step 1: Identify the standard enthalpy of formation (ΔHf°) values
We are given the following standard enthalpy of formation values:
- ΔHf° of \(Fe_{2}O_{3}\) = -8242 kJ/mol
- ΔHf° of \(CO_{2}\) = -393.7 kJ/mol

### Step 2: Write the formula for calculating ΔH
The enthalpy change for the reaction can be calculated using the formula:
\[ \Delta H = \sum (N \cdot \Delta Hf° \text{ of products}) - \sum (N \cdot \Delta Hf° \text{ of reactants}) \]

### Step 3: Identify the coefficients from the balanced equation
From the balanced equation:
- Products:
- 4 moles of \(Fe\) (ΔHf° = 0 for elements in their standard state)
- 3 moles of \(CO_{2}\)
- Reactants:
- 2 moles of \(Fe_{2}O_{3}\)
- 3 moles of \(C\) (ΔHf° = 0 for elements in their standard state)

### Step 4: Substitute the values into the formula
Since the ΔHf° for \(Fe\) and \(C\) is 0, we can simplify the equation:
\[ \Delta H = [4 \cdot 0 + 3 \cdot (-393.7)] - [2 \cdot (-8242) + 3 \cdot 0] \]

Calculating this gives:
\[ \Delta H = [0 - 1181.1] - [-16484] \]
\[ \Delta H = -1181.1 + 16484 \]
\[ \Delta H = 467.3 \, \text{kJ/mol} \]

### Step 5: Determine the nature of the reaction
Since ΔH is positive (467.3 kJ/mol), this indicates that the reaction absorbs heat from the surroundings.

### Conclusion
Thus, the reaction is **endothermic**.