The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given by 

\Delta _{r}G^{o}=A-BT

Where A and B are non -zero constants. Which of the following is TRUE about this reaction ?

  • Option 1)

    Endothermic if A < 0 and B > 0 

  • Option 2)

    Exothermic if B < 0

  • Option 3)

    Exothermic if A > 0 and B < 0

  • Option 4)

    Endothermic if A > 0

Answers (1)
A admin

 

Gibb's free energy (Δ G) -

\Delta G= \Delta H-T \Delta S
 

- wherein

\Delta G= Gibb's free energy

\Delta H= enthalpy of reaction

\Delta S= entropy

T= temperature

 

 

Δ G of equilibrium -

\Delta G_{0}= -2.303 RT \log K_{c}
 

- wherein

At Equilibrum    

\Delta G= 0

and Q= K_{c}

 

 

Spontanous process -

\Delta G=\Delta H-T\Delta S

 

- wherein

For spontanouse process \Delta G must be negative.

Formula 

\Delta G=A-BT

=\Delta H-T\Delta S

A=\Delta H

\Delta H=A=+ve\; \: endothermic

 


Option 1)

Endothermic if A < 0 and B > 0 

Option 2)

Exothermic if B < 0

Option 3)

Exothermic if A > 0 and B < 0

Option 4)

Endothermic if A > 0

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