Sulphur exists in more than one solid form. The stable form at room temperature is rhombic sulphur. But above room temperature the following reaction occurs :
S (rhombic) `rarr` S (monoclinic)
If `Delta H = 276.144` J at 298 K and 1 atm and `Delta G = 75.312 J`
Assume that `Delta H` and `Delta S` do not vary significantly with temperature, calculate `T_(eq)`, the temperature at which rhombic and monoclinic sulphur exist in equilibrium with each other.

Explanation

To solve the problem of finding the equilibrium temperature \( T_{eq} \) at which rhombic sulfur and monoclinic sulfur exist in equilibrium, we can follow these steps:

### Step 1: Understand the relationship between ΔG, ΔH, and ΔS
The Gibbs free energy change (ΔG) for a reaction is given by the equation:
\[ \Delta G = \Delta H - T \Delta S \]
At equilibrium, ΔG = 0. Therefore, we can rearrange the equation to find the equilibrium temperature \( T_{eq} \):
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