1. Hess's law states that the overall enthalpy change of a chemical process is independent of the path taken.
2. The document uses the reaction of sodium hydroxide and hydrochloric acid to illustrate Hess's law. It shows that the enthalpy change of the direct reaction is equal to the sum of the enthalpy changes for the stepwise reactions.
3. Representing the reactions on an enthalpy level diagram and enthalpy cycle confirms that Hess's law applies, with the enthalpy change for the overall reaction being the sum of the enthalpy changes for the individual steps.
Redox Reaction and Electrochemical Cell (Reaksi Redoks dan Sel Elektrokimia)DindaKamaliya
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An electrochemical cell converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells separated by a salt bridge. In the cathode half-cell, reduction occurs as oxidized species gain electrons. In the anode half-cell, oxidation occurs as reduced species lose electrons. Electrons flow through an external circuit from the anode to the cathode. The standard electrode potential of each half-reaction predicts the cell's voltage under standard conditions.
1. Hess's law states that the overall enthalpy change of a chemical process is independent of the path taken.
2. The document uses the reaction of sodium hydroxide and hydrochloric acid to illustrate Hess's law. It shows that the enthalpy change of the direct reaction is equal to the sum of the enthalpy changes for the stepwise reactions.
3. Representing the reactions on an enthalpy level diagram and enthalpy cycle confirms that Hess's law applies, with the enthalpy change for the overall reaction being the sum of the enthalpy changes for the individual steps.
Redox Reaction and Electrochemical Cell (Reaksi Redoks dan Sel Elektrokimia)DindaKamaliya
?
An electrochemical cell converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells separated by a salt bridge. In the cathode half-cell, reduction occurs as oxidized species gain electrons. In the anode half-cell, oxidation occurs as reduced species lose electrons. Electrons flow through an external circuit from the anode to the cathode. The standard electrode potential of each half-reaction predicts the cell's voltage under standard conditions.