The $E^{\ominus}$ for $Cl_{2}/Cl^{-}$ is $+1.36 \ V,$ for $I_{2}/I^{-}$ is $+0.53 \ V,$ for $Ag^{+}/Ag$ is $+0.79 \ V,$ $Na^{+}/Na$ is $-2.71 \ V$ and for $Li^{+}/Li$ is $-3.04 \ V.$ Arrange the following ionic species in decreasing order of reducing strength: $I^{-}, Ag, Cl^{-}, Li, Na$
(A) Reducing strength is inversely proportional to the standard reduction potential $(E^{\ominus})$.
Lower (more negative) $E^{\ominus}$ values indicate stronger reducing agents.
The given $E^{\ominus}$ values are:
$Li^{+}/Li = -3.04 \ V$
$Na^{+}/Na = -2.71 \ V$
$I_{2}/I^{-} = +0.53 \ V$
$Ag^{+}/Ag = +0.79 \ V$
$Cl_{2}/Cl^{-} = +1.36 \ V$
Arranging these in decreasing order of reducing strength (from most negative $E^{\ominus}$ to most positive $E^{\ominus}$):
$Li > Na > I^{-} > Ag > Cl^{-}$
Lower (more negative) $E^{\ominus}$ values indicate stronger reducing agents.
The given $E^{\ominus}$ values are:
$Li^{+}/Li = -3.04 \ V$
$Na^{+}/Na = -2.71 \ V$
$I_{2}/I^{-} = +0.53 \ V$
$Ag^{+}/Ag = +0.79 \ V$
$Cl_{2}/Cl^{-} = +1.36 \ V$
Arranging these in decreasing order of reducing strength (from most negative $E^{\ominus}$ to most positive $E^{\ominus}$):
$Li > Na > I^{-} > Ag > Cl^{-}$
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The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.
MediumAIPMT 1993
View SolutionGiven:
$E^o_{Cr^{3+}/Cr} = -0.74 \ V$,$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V$,$E^o_{Cl_2/Cl^{-}} = 1.36 \ V$
Based on the data given above,the strongest oxidising agent will be:
$E^o_{Cr^{3+}/Cr} = -0.74 \ V$,$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V$,$E^o_{Cl_2/Cl^{-}} = 1.36 \ V$
Based on the data given above,the strongest oxidising agent will be:
DifficultJEE MAIN 2013
View SolutionStandard electrode potential for $Sn^{4+}/Sn^{2+}$ couple is $+0.15 \ V$ and that for the $Cr^{3+}/Cr$ couple is $-0.74 \ V.$ These two couples in their standard state are connected to make a cell. The cell potential will be ........ $V$
DifficultAIPMT 2011
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Easy
View SolutionStandard reduction potentials of the half-reactions are given below:
$F_{2(g)} + 2e^- \rightarrow 2F^-_{(aq)}$; $E^o = +2.85 \ V$
$Cl_{2(g)} + 2e^- \rightarrow 2Cl^-_{(aq)}$; $E^o = +1.36 \ V$
$Br_{2(l)} + 2e^- \rightarrow 2Br^-_{(aq)}$; $E^o = +1.06 \ V$
$I_{2(s)} + 2e^- \rightarrow 2I^-_{(aq)}$; $E^o = +0.53 \ V$
The strongest oxidising and reducing agents respectively are:
$F_{2(g)} + 2e^- \rightarrow 2F^-_{(aq)}$; $E^o = +2.85 \ V$
$Cl_{2(g)} + 2e^- \rightarrow 2Cl^-_{(aq)}$; $E^o = +1.36 \ V$
$Br_{2(l)} + 2e^- \rightarrow 2Br^-_{(aq)}$; $E^o = +1.06 \ V$
$I_{2(s)} + 2e^- \rightarrow 2I^-_{(aq)}$; $E^o = +0.53 \ V$
The strongest oxidising and reducing agents respectively are:
MediumAIPMT 2012
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