JEE Mains · Chemistry · STD 12 - 2. Electrochemistry
For a general redox reaction
Anode : \(\text{Red}_1 \rightarrow \text{Ox}_1^{n_1^+} + n_1 e^-\)
Cathode : \(\text{Ox}_2 + n_2 e^- \rightarrow \text{Red}_2^{n_2^-}\)
Which of the following statement is incorrect ?
- A The overall reaction can be written as \(n_2\text{Red}_1 + n_1\text{Ox}_2 \rightleftharpoons n_2\text{Ox}_1^{n_1^+} + n_1\text{Red}_2^{n_2^-}\)
- B The electrons do not appear in the overall reaction because electrons produced at the anode are consumed at the cathode.
- C Here \(n\) is the number of electrons transferred in redox reaction.
- D If the reaction is carried out reversibly, the electrical work done is equal to the ratio of charge and potential difference through which charge is moved.
Answer & Solution
Correct Answer
(D) If the reaction is carried out reversibly, the electrical work done is equal to the ratio of charge and potential difference through which charge is moved.
Step-by-step Solution
Detailed explanation
For the given redox reaction, the half-cell reactions are: Anode: \(\text{Red}_1 \rightarrow \text{Ox}_1^{n_1^+} + n_1 e^-\) Cathode: \(\text{Ox}_2 + n_2 e^- \rightarrow \text{Red}_2^{n_2^-}\) To obtain the overall balanced chemical equation, we multiply the anode reaction by…
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