For the reaction, X (s) Y (s)+ Z (g) , the plot of p_ Z p^ versus 10⁴ T is given below (in solid line), where p_ Z is the pressure (in bar) of the gas Z at temperature T and p^ =1 bar. (Given, d ( K) d ( 1 T ) =- H^ R , where the equilibrium constant, K= p_ z p^ and the gas constant, R =8.314 ~J ~K ⁻¹ ~mol ⁻¹ ) The value of ∆ S o (in kJ mol - 1 ) for the given reaction, at 1000 K is ___.

Step-by-step solution

According to graph when T = 1000   K and 10 4 T = 10 then ln p z p ϕ = − 3 Now, ΔG o = ΔH o − T   ΔS o − RT   lnK p = ΔH o − T   ΔS o R   ln   K p = ΔS o − ΔH o T ΔS o = RlnK p + ΔH o T lnK p = ln p z p ϕ = − 3 ΔS o = − 3 R + 166 .28 × 10 3 J 1000 166 .28 − 3 × 8 .314 ΔS o = 141 .34