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Consider the reaction: N2(g) + 3 F2(g) → 2 NF3(g) ΔH° = -249 kJ and ΔS° = -278 J/K at 25°C Calculate ΔG° and state whether the equilibrium composition should favor reactants or products at standard conditions.

Respuesta :

Answer : The value of [tex]\Delta G^o[/tex]  is -166156 J and equilibrium composition should favor products at standard conditions.

Explanation :

Now we have to calculate the Gibbs free energy.

As we know that,

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

where,

[tex]\Delta G^o[/tex] = standard Gibbs free energy  = ?

[tex]\Delta H^o[/tex] = standard enthalpy = -249 kJ = -249000 J

[tex]\Delta S^o[/tex] = standard entropy = -278 J/K

T = temperature of reaction = [tex]25^oC=273+25=298K[/tex]

Now put all the given values in the above formula, we get:

[tex]\Delta G^o=(-249000J)-(298K\times -278J/K)[/tex]

[tex]\Delta G^o=-166156J[/tex]

  • A reaction to be spontaneous when [tex]\Delta G<0[/tex]  and reaction will be favored in the forward direction that means favored in products.
  • A reaction to be non-spontaneous when [tex]\Delta G>0[/tex]  and reaction will be favored in the backward direction that means favored in reactants.

As the value of [tex]\Delta G[/tex] is less than zero that means the reaction is spontaneous and reaction will be favored in the forward direction that means favored in products.

Hence, the value of [tex]\Delta G^o[/tex]  is -166156 J and equilibrium composition should favor products at standard conditions.

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