Question Title: Thermodynamic Sign Predictions for Various Chemical Processes---**Objective:**Evaluate the expected signs for changes in Gibbs free energy (ΔG°), enthalpy (ΔH°), and entropy (ΔS°) for each of the following processes, with explanations for each prediction.---**Processes:**1. **Electrolysis of water to give gaseous hydrogen and oxygen:** - Predict the thermodynamic signs for ΔG°, ΔH°, and ΔS°. - Provide an explanation based on the nature of electrolysis as an endothermic, non-spontaneous process, resulting in increased disorder due to gas formation.2. **Dissolving a small amount of sodium nitrate in water (the solution becomes cold):** - Predict the signs for ΔG°, ΔH°, and ΔS°. - Explain how the endothermic nature of the process (indicated by the cooling effect) and the increase in disorder affect these thermodynamic values.3. **Combustion of wood:** - Determine the expected signs for ΔG°, ΔH°, and ΔS°. - Discuss how the exothermic release of energy and increased disorder from gaseous product formation influence these values.---This exercise helps in understanding the relationship between chemical processes and their thermodynamic properties, which is crucial for predicting the spontaneity and behavior of reactions.

Enthalpy change is the name given to the amount of heat evolved or absorbed in a reaction carried out at constant pressure. Entropy, S, is a state function and is a measure of disorder or randomness. Gibbs free energy combines enthalpy and entropy into a single value. Gibbs free energy is the energy associated with a chemical reaction that can do useful work. It equals the enthalpy minus the product of the temperature and entropy of the system. G = H – TS At constant temperature ΔG = ΔH – TΔS ΔG predicts the direction of a chemical reaction. If ΔG is negative, then the reaction is spontaneous. If ΔG is positive, then the reaction is non-spontaneous ∆H ∆S ∆G comments on reaction - + - spontaneous + + + or- spontaneous at high temperature - - + or - spontaneous at low temperature + - + non-spontaneousa) Electrolysis of water to give gaseous hydrogen and oxygen occur at -1.229V standard electrode potential. Since the value of electrode potential is negative then Gibb's energy is positive by the reaction: ∆G=-nF∆Eocell Also the electrolysis required at least 286KJ of electric energy for reaction to proceed , thus enthalpy change is positive . In order for reaction to be spontaneous entropy should be positive at high temperature. Thus ∆H=+ve∆G=+ve∆S=+veb) Addition of small amount of sodium nitrate to water make the solution cold . It occurs due to the fact that energy is being absorbed from the surrounding. Thus reaction is endothermic and value of enthalpy change is positive. For reaction to be spontaneous Gibb's energy is negative and entropy is then positive. ∆H=+ve∆G=-ve∆S=+vec) Combustion of wood release energy , thus it is a exothermic reaction. So enthalpy change of reaction is negative. Since it is spontaneous reaction Gibb's energy is negative and entropy positive. ∆H=-ve∆G=-ve∆S=+ve