The enthalpy of vaporization (δh°vap) of benzene is 30.7 kj/mol at its normal boiling point of 353.3 k. what is δs°vap at this temperature? a. 383 j/(mol·k) b. 0.0115 j/(mol·k) c. 86.9 j/(mol·k) d. 0.087 j/(mol·k) e. 11.5 j/(mol·k)

The correct answer is Option c.

Explanation:

Vaporization is defined as the physical process in which liquid particles get converted to gaseous particles.

The value of standard Gibbs free energy is 0 for equilibrium reactions.

To calculate for the reaction, we use the equation:

where,

= standard entropy change of vaporization

= standard enthalpy change of vaporization = 30.7 kJ/mol = 30700 J/mol    (Conversion factor: 1 kJ = 1000 J)

T = temperature of the reaction = 353.3 K

Putting values in above equation, we get:

Hence, the correct answer is Option c.