Gibbs Free Energy

To find the change in Gibbs free energy for the reaction, we use the following equation: Where: - is the change in enthalpy, - is the change in entropy, - is the temperature in Kelvin. ### Step 1: Convert temperature to Kelvin The temperature is given as , which is: ### Step 2: Calculate The change in entropy is given as . To calculate , we need the enthalpy change . For the phase change from liquid to gas, is typically at . Now, calculate: Thus, the value of is:

First calculate : Given: So, Now use: Given: Thus,
Hence, the correct answer is:

Concept: Chemistry - Gibbs Free Energy. [ \Delta G=\Delta H-T\Delta S ]
Step 1: Convert entropy unit. [ \Delta S=-45\text{ J K}^{-1}\text{mol}^{-1}=-0.045\text{ kJ K}^{-1}\text{mol}^{-1} ]
Step 2: Substitute values. [ \Delta G=-13-298(-0.045) ]
Step 3: Calculate. [ \Delta G=-13+13.41=0.41 ] [ \Delta G=+0.41\text{ kJ mol}^{-1} ]
Step 4: Final answer. [ \boxed{+0.41\text{ kJ mol}^{-1}} ]
Hence, correct option is (C).