Physical Chemistry - Gibbs Free Energy

In an exergonic reaction, products will have __________ Gibbs free energy and the reaction is __________.

For Constant Temperature, Gibbs Free Energy is defined as:

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

Where , $\small \Delta G$ is the change in Gibbs Free Energy, $\small \Delta H$ is the change in enthalpy, $\small T$ is temperature, and $\small \Delta S$ is the change in entropy.

Which of the following scenarios is not possible?

The enthalpy of a reaction is $35\frac{kJ}{mol}$ and the entropy of a reaction is $3\frac{J}{mol\cdot K}$ . Which of the following is the Gibbs free energy (in $\frac{kJ}{mol}$ ) of this reaction?

For constant temperature, Gibbs free energy is defined as:

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

Where , $\small \Delta G$ is the change in Gibbs free energy, $\small \Delta H$ is the change in enthalpy, $\small T$ is temperature, and $\small \Delta S$ is the change in entropy.

Given that a system is spontaneous, which of the following states are possible?

I. $\Delta G<0, \Delta S>0, \Delta H<0$

II. $\Delta G<0, \Delta S<0, \Delta H>0$

III. $\Delta G<0, \Delta S>0, \Delta H>0$

IV. $\Delta G>0, \Delta S<0, \Delta H>0$

Gibbs Free Energy

Practice Questions