The cell reaction for a galvanic cell is given below:
Zn(s) + 2Ag+
(aq) →Zn2+ (aq) + 2Ag(s)
i) Write the half-cell reactions at the anode and the cathode.
ii) Calculate the value of cell emf under standard conditions; use data from Table 7.1.
iii) Will the reaction be spontaneous as written?
i) Oxidation at anode: "Zn(s) \u2192 Zn^{2+} (aq) + 2e^{\u2212}"
Reduction at cathode: "Ag+ (aq) + e^{\u2212} \u2192 Ag (s)"
ii)Ag: E = +0.80 V
Zn: E = -0.76 V
"E_0cell = E_0cath \u2013 E_0anode = +0.80 \u2013(-0.76) = 1.56 V"
iii)"\u0394G = -nFE"
If "E_0" is positive, ΔG is negative, thus reaction is spontaneous.
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