The standard oxidation potentials of zinc and | vedclass

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(A) For a reaction to be spontaneous,the standard cell potential $E^o_{cell}$ must be positive.$E^o_{cell} = E^o_{ox}(	ext{anode}) + E^o_{red}(	ext{

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$Zn_{(s)} + 2Ag^{+}_{(aq)} 	o Zn^{2+}_{(aq)} + 2Ag_{(s)}$

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(A) For a reaction to be spontaneous,the standard cell potential $E^o_{cell}$ must be positive.$E^o_{cell} = E^o_{ox}(	ext{anode}) + E^o_{red}(	ext{cathode})$Alternatively,$E^o_{cell} = E^o_{ox}(	ext{anode}) - E^o_{ox}(	ext{cathode})$.For the reaction $Zn_{(s)} + 2Ag^{+}_{(aq)} 	o Zn^{2+}_{(aq)} + 2Ag_{(s)}$:$Zn$ is oxidized $(E^o_{ox} = 0.76 \ V)$ and $Ag^+$ is reduced $(E^o_{red} = -E^o_{ox} = 0.80 \ V)$.$E^o_{cell} = 0.76 \ V + 0.80 \ V = 1.56 \ V$.Since $E^o_{cell} > 0$,the reaction is spontaneous. In this reaction,$Zn$ acts as the anode and $Ag$ acts as the cathode.

The standard oxidation potentials of zinc and silver in water at $298 \ K$ are:
$Zn_{(s)} \to Zn^{2+}_{(aq)} + 2e^- ; E^o_{ox} = 0.76 \ V$
$Ag_{(s)} \to Ag^{+}_{(aq)} + e^- ; E^o_{ox} = -0.80 \ V$
Which of the following reactions actually takes place spontaneously?

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The standard oxidation potentials of zinc and silver in water at $298 \ K$ are:$Zn_{(s)} \to Zn^{2+}_{(aq)} + 2e^- ; E^o_{ox} = 0.76 \ V$$Ag_{(s)} \to Ag^{+}_{(aq)} + e^- ; E^o_{ox} = -0.80 \ V$Which of the following reactions actually takes place spontaneously?