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Sulphur exists in more than one solid fo...

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") rarrS("monoclinic")`
If `DeltaH^(Theta) = 276.144J at 298 K` and `1atm` and `DeltaG^(Theta) = 75.312J`
a. Calculate `DeltaS^(Theta)` at `298K`.
b. Assume that `DeltaH^(Theta)` and `DeltaS^(Theta)` do not vary significantly with temperature, calculate `T_(eq)`, the temperature at which rhombic and monoclinic sulphur exist in equilibrium with each other.

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To solve the problem, we will break it down into two parts as outlined in the question. ### Part (a): Calculate ΔS° at 298 K We know from thermodynamics that the relationship between Gibbs free energy (ΔG), enthalpy (ΔH), and entropy (ΔS) is given by the equation: \[ \Delta G = \Delta H - T \Delta S ...
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Sulphur exists is more than one solid form. The stable form at room temperature is rhombic sulphur. But above room temperature the following reaction occurs. S ("rhomic") rarrS("monoclinic") If DeltaH^(Theta) =- 276.144J at 298 K and 1atm and DeltaG^(Theta) = 75.312J a. Calculate DeltaS^(Theta) at 298K .

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.

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