Recent activity by SueFcg023218

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Given the following electrochemical equation:Cu(s) | Cu²⁺(aq, 0.0100 M) || Cr³⁺(aq, 1.00 M) | Cr(s)At 298 K, the standard reduction potential for Cu²⁺/Cu is +0.34 V and for Cr³⁺/Cr is -0.74 V. Calculate the equilibrium constant (K) for the above electrochemical reaction.

answered 23 hours ago in ElectroChemistry

1 answer 45 views

A student needs to calculate the maximum electrical work that can be obtained from an electrochemical cell of standard hydrogen electrode (SHE) potential -0.76 V and a zinc electrode potential of -0.46 V, when 0.5 moles of zinc metal is oxidized to form zinc ions at 25 °C. Assume that the Faraday constant is 96,485 Coulombs per mole of electrons and the gas constant is 8.314 J/mole.K.

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