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.

$Zn \rightarrow Zn^{2+} + 2e^-$	$E^{\circ} = +0.76 \ V$
$Fe \rightarrow Fe^{2+} + 2e^-$	$E^{\circ} = +0.41 \ V$

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?

Similar Questions

The standard reduction potentials for $Al^{3+} | Al$,$Fe^{2+} | Fe$,and $Br_2 | Br^-$ are $-1.66 \ V$,$-0.45 \ V$,and $1.09 \ V$ respectively. What is the correct order of their reducing power?

Calculate the $Zn-Cu$ cell (Daniell cell) potential. Given: $E^o_{Zn^{2+}|Zn} = -0.76 \ V$ and $E^o_{Cu^{2+}|Cu} = 0.34 \ V$. (in $V$)

The correct order of reduction potentials of the following pairs is
$A.$ $Cl_2 / Cl^{-}$
$B.$ $I_2 / I^{-}$
$C.$ $Ag^{+} / Ag$
$D.$ $Na^{+} / Na$
$E.$ $Li^{+} / Li$
Choose the correct answer from the options given below.

What is the standard cell potential for the cell $Zn | Zn^{2+} (1M) || Cu^{2+} (1M) | Cu$? Given $E^o$ for $Zn^{2+} | Zn = -0.76 \ V$ and $E^o$ for $Cu^{2+} | Cu = +0.34 \ V$.

The standard reduction potential $E^{\circ}$ for half reactions are
$Zn \rightarrow Zn^{2+} + 2e^-$ $E^{\circ} = +0.76 \ V$
$Fe \rightarrow Fe^{2+} + 2e^-$ $E^{\circ} = +0.41 \ V$

The $EMF$ of the cell reaction $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ is

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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?