contestada

For a given reaction, ΔS = +106 J/mol ⋅ K, and the reaction is spontaneous at temperatures above the crossover temperature, 446 K. The value of ΔH = _______ kJ/mol, assuming that ΔH and ΔS do not vary with temperature.

Respuesta :

Answer:  47.276 kJ/mol

Explanation:

According to Gibb's equation:

[tex]\Delta G=\Delta H-T\Delta S[/tex]

[tex]\Delta G[/tex] = Gibbs free energy  

[tex]\Delta H[/tex] = enthalpy change

[tex]\Delta S[/tex] = entropy change  = +106 J/mol

T = temperature in Kelvin  = 446 K

[tex]\Delta G[/tex]= +ve, reaction is non spontaneous

[tex]\Delta G[/tex]= -ve, reaction is spontaneous

[tex]\Delta G[/tex]= 0, reaction is in equilibrium

[tex]\Delta H=T\Delta S[/tex]

[tex]\Delta H=T\Delta S[/tex]

[tex]\Delta H=446K\times +106J/Kmol=47276J/mol=47.276kJ/mol[/tex]   (1kJ=1000J)

Thus the value of ΔH = 47.276 kJ/mol, assuming that ΔH and ΔS do not vary with temperature.

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