The standard Gibbs energy for the given cell reaction in $kJ \, mol^{-1}$ at $298 \, K$ is $Zn_{(s)} + Cu^{2+}_{(aq)} \to Zn^{2+}_{(aq)} + Cu_{(s)}$,given $E^o = 2 \, V$ at $298 \, K$ [Faraday's constant $F = 96500 \, C \, mol^{-1}$].
- A$-192$
- B$384$
- C$-384$
- D$192$
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Similar Questions
Which of the following will have a standard oxidation potential less than $SHE$?
Difficult
View SolutionAmong $Mg$,$Cu$,$Fe$,and $Zn$,the metal that does not produce hydrogen gas in reaction with hydrochloric acid is:
MediumKVPY 2015
View Solution$Zn^{2+} + 2e^- \to Zn_{(s)}$; $E^o = -0.76 \ V$
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = +0.77 \ V$
$Cr^{3+} + 3e^- \to Cr_{(s)}$; $E^o = -0.74 \ V$
$H^{+} + e^- \to 1/2 H_2$; $E^o = 0.00 \ V$
Which of the following is the strongest reducing agent?
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = +0.77 \ V$
$Cr^{3+} + 3e^- \to Cr_{(s)}$; $E^o = -0.74 \ V$
$H^{+} + e^- \to 1/2 H_2$; $E^o = 0.00 \ V$
Which of the following is the strongest reducing agent?
Easy
View SolutionFor the following cell,the standard electrode potential $E_{cell}^0$ is . . . . . . .
$E_{Zn^{2+}/Zn}^0 = -0.76 \ V, E_{Cu^{2+}/Cu}^0 = 0.34 \ V$
$Zn | Zn^{2+} || Cu^{2+} | Cu$ (in $V$)
$E_{Zn^{2+}/Zn}^0 = -0.76 \ V, E_{Cu^{2+}/Cu}^0 = 0.34 \ V$
$Zn | Zn^{2+} || Cu^{2+} | Cu$ (in $V$)
For the cell reaction $Mg_{(s)} + Zn^{2+}_{(aq)} (1M) \rightarrow Zn_{(s)} + Mg^{2+}_{(aq)} (1M)$,the $emf$ is $1.60 \ V$. The $E$ of the cell is ........ $V$.
Medium
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