In a galvanic cell, a spontaneous redox reaction occurs. However, the reactants

Question

In a galvanic cell, a spontaneous redox reaction occurs. However, the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting cell potential is measured in volts (V) and is defined by the equation given below: E_cell degree = E_rod^degree (cathode) - E_rod^degree (anode) A table of standard reduction potentials gives E_rod^degree values tor common half-reactions. Calculate the standard potential for the following galvanic cell Zn(s) | Zu^2+ (aq) || Ag^+ (aq) | Ag(s) which has the overall balanced equation: Zn(s) + 2Ag^+ (aq) rightarrow Zn^2+ (aq) + 2Ag(s) Express your answer to three significant figures and include the appropriate units. In the context of the zinc-siver cell described in match each of the following descriptions to the anode or cathode. Drag the appropriate items to their respective bins.

Explanation / Answer

Here Zn system is the anode and Ag system is the cathode

therefore standard cell potential = Ecathode - Eanode = 0.80 - (-0.76) = 1.56 volts

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