Students calculated the cell voltage for the reaction, π΅π2 + 2πππΆπ βΆ 2πππ΅π + πΆπ2 through the formula πΈΒ°ππππ= πΈΒ°πππ+ πΈΒ°ππ₯π the answer was negative. It means that:
Correct answer: B. The reaction is non spontaneous and not feasible
- A. The reaction is non spontaneous and feasible
- B. The reaction is non spontaneous and not feasible
- C. The reaction is spontaneous and feasible
- D. The reaction is spontaneous and not feasible
Explanation
The energy associated with the separation/transfer of charge is the property of potential, E. A cell potential's arithmetic sign determines the spontaneity of the cell reaction, with positive values indicating spontaneous and feasible reactions and zero or negative values indicating nonspontaneous and non-feasible reactions (spontaneous in the reverse direction). If the value is positive, the oxidation-reduction reaction is spontaneous. Only spontaneous reactions are feasible. That is, without the assistance of a third party. The cathode undergoes reduction, while the anode undergoes oxidation. If the value is negative, it signifies that only the opposite reaction is spontaneous. It refers to the cathode's oxidation and the anode's reduction. The change in Gibbs free energy in a galvanic cell, where a spontaneous redox reaction drives the cell to produce an electric potential, must be negative. The cell potential, which is positive when electrons flow freely through the electrochemical cell, is the polar opposite of this.
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Electrochemistry describes electron transfer through oxidation and reduction, identifies oxidizing and reducing agents, and applies oxidation numbers to balance redox equations. It also covers electrode potential and the standard hydrogen electrode, which provides the reference for comparing the reduction tendencies of other electrodes.
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