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") 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.

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.

What is the equilibrium constant K_(c) for the following reaction at 400K ? 2NOCI(g) hArr 2NO(g) +CI_(2)(g) DeltaH^(Theta) = 77.2 kJ mol^(-1) and DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K .

Calculated the equilibrium constant for the following reaction at 298K : 2H_(2)O(l) rarr 2H_(2)(g) +O_(2)(g) Delta_(f)G^(Theta) (H_(2)O) =- 237.2 kJ mol^(-1),R = 8.314 J mol^(-1) K^(-1)

For a demerization reaction , 2A (g) to A_2 (g) at 298 K, Delta U(Theta) = - 20 kJ"mol"^(-1), Delta S^(Theta) = - 30 JK^(-1) "mol"^(-1) , then the Delta G^(Theta) will be _________J.

Calculate the equilibrium constnat for the reaction given below at 400K , if DeltaH^(Theta) = 77.2 kJ "mole"^(-1) and DeltaS^(Theta) = 122 J K^(-1) "mole"^(-1) . PCI_(5)(g) rarr PCI_(3)(g) +CI_(2)(g)

Calculate equilibrium constant for the reaction given below at 400K , if DeltaH^(Theta) = 77.2 kJ mol^(-1) and DeltaS^(Theta) = 122 J K^(-1) mol^(-1) PCI_(5)(g) rarr PCI_(3)(g) +CI_(2)(g)

The temperature dependence of equilibrium constant of a reaction is given by ln K_(eq) = 4.8 -(2059)/(T) . Find Delta_(r)G^(Theta), Delta_(r)H^(Theta), Delta_(r)S^(Theta) at 298 K

Predict whether it is possible or not to reduce magnesium oxide using carbon at 298K according to the reaction. MgO(s) +C(s) rarr Mg(s) +CO(g) Delta_(r)H^(Theta) = +491.18 kJ mol^(-1) and Delta_(r)S^(Theta) = 197.67 J K^(-1) mol^(-1) If not at what temperature, the reaction becomes spontaneous.

The standard Gibbs energy change value (Delta_(r)G^(Theta)) at 1773K are given for the following reactions: 4Fe +3O_(2) rarr 2Fe_(2)O_(3), Delta_(r)G^(Theta) = - 1487 kJ mol^(-1) 4AI +3O_(2) rarr 2AI_(2)O_(3),Delta_(r)G^(Theta) =- 22500 kJ mol^(-1) 2CO +O_(2) rarr 2CO_(2),Delta_(r)G^(Theta) =- 515 kJ mol^(-1) Find out the possibility of reducing Fe_(2)O_(3) and AI_(2)O_(3) with CO at this temperature.