Given the following thermochemical equations `:`
(i) S( rhombic ) `+ O_(2)(g) rarr SO_(2)(g) , Delta H = - 297.5 kJ mol^(-1)`
(ii) S ( monoclinic) `+ O_(2) rarr SO_(2)(g) , Delta H = - 300.0 kJ mol^(-1)`
Calculate `Delta H ` for the transformation of one gram atomof rhombic sulphur into monochlinic sulphur.

Explanation

To calculate the change in enthalpy (ΔH) for the transformation of one gram atom of rhombic sulfur (S_rhombic) into monoclinic sulfur (S_monoclinic), we can use the provided thermochemical equations. Here’s a step-by-step solution:

### Step 1: Write down the given thermochemical equations
1. **For rhombic sulfur:**
\[ \text{S (rhombic)} + \text{O}_2(g) \rightarrow \text{SO}_2(g), \quad \Delta H = -297.5 \, \text{kJ/mol} \]
2. **For monoclinic sulfur:**
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