The standard electrode potential (E∘) for Daniel cell is +1.1V. Calculate ΔG∘ for the reaction. Zn(s)+Cu2+(aq)→Zn2+(aq)+Cu(s) (1F=96500C/mol)
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Solution
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ΔG=−nFE =−2×96500×2.2 =−212300J =−212.3kJ
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Similar Questions
Q1
The standard electrode potential (E∘) for Daniel cell is +1.1V. Calculate ΔG∘ for the reaction. Zn(s)+Cu2+(aq)→Zn2+(aq)+Cu(s) (1F=96500C/mol)
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Q2
The standard electrode potential (E∘) for Daniel cell is + 1. 1 V. Calculate the ΔG∘ for the reaction Zn(s)+Cu2+(aq)⟶Zn2+(aq)+Cu(s) (1F=96500Cmol−1).
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Q3
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Q4
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Q5
The standard electrode potential of a Daniell cell is 1.1V. Find the standard Gibbs energy for the reaction. Zn(s)+Cu2+(aq.)→Zn2+(aq.)+Cu(s)