I. MODIFIED TRUE OR FALSE. Write TRUE if the statement is always correct. If the statement is false, correct the underlined word$/$s to make the statement true. $2$ points each

I. In all cases, the deviations of the behavior of the solution from ideal is given by the property changes in mixing.

$2.$ In an ideal solution, the activity coefficient of species $i$ is equal to zero.

$3.$ At equilibrium, the Gibbs free energy is maximized.

$4.$ At chemical equilibrium, the sum of the product of chemical potential and fugacity of species $i$ is zero.

$5.$ For real solutions, the entropy change of mixing is zero.

$6.$ Lewis$/$Randall Rule states that the fugacity coefficient of each species in an ideal solution is proportional to its mole fraction.

$7.$ For pure species, the entropy change of mixing is non$-$zero

$3.$ The Gibbs free energy change of mixing of ideal solutions is

zero.

$9.$ In ideal solutions, the chemical potential of species $i$ is a function of temperature, pressure, and volume.

$10.$ The partial molar enthalpy of an ideal solution is equal to the sum of the products of mole fractions of each component and the corresponding pure species enthalpies.

The fugacity is$\_$a factor that is introduced to the Raoult's Law to account for liquid$-$phase non$-$idealities.

For ideal solutions, the partial excess entropy of species $i$ is zero.

In the three$-$phase point $($vapor$/$liquid$/$liquid equilibrium$)$ with two non$-$reacting species, the of degree$/$s of freedom is zero.

In a real solution, the enthalpy change of mixing is equal to the residual molar enthalpy.

In real solutions, the volume change of mixing is equal to the partial molar volume of pure species $i.$