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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)

best_answer

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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