The values of E0 of some electrode reactions are given below I2 + 2e−→ 2I− E0=0.54 voltsSn+4 + 2e−→ Sn2+ E0= 0.152 voltsCl2 + 2e− → 2Cl− E0= 1.36 voltsFe+3 + e− →Fe2+ E0= 0.76 voltsCe+4 + e− → Ce3+ E0= 1.6 voltsChoose the correct statement(s)

Fe3++Ce3+→Ce4++Fe2+ EO<0 I2+Cl−→Cl2+I− EO<0

The values of E0 of some electrode reactions are given below I2 + 2e−→ 2I− E0=0.54 voltsSn+4 + 2e−→ Sn2+ E0= 0.152 voltsCl2 + 2e− → 2Cl− E0= 1.36 voltsFe+3 + e− →Fe2+ E0= 0.76 voltsCe+4 + e− → Ce3+ E0= 1.6 voltsChoose the correct statement(s)

Fe3++Ce3+→Ce4++Fe2+ EO<0 I2+Cl−→Cl2+I− EO<0

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The values of $E_{0}$ of some electrode reactions are given below
$\begin{array}{l} I_{2} + 2 e^{-} \to 2 I^{-} E_{0} = 0.54 v o l t s \\ S n^{+ 4} + 2 e^{-} \to S n^{2 +} E_{0} = 0.152 v o l t s \\ C l_{2} + 2 e^{-} \to 2 C l^{-} E_{0} = 1.36 v o l t s \\ F e^{+ 3} + e^{-} \to F e^{2 +} E_{0} = 0.76 v o l t s \\ C e^{+ 4} + e^{-} \to C e^{3 +} E_{0} = 1.6 v o l t s \end{array}$
Choose the correct statement(s)

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$S n^{2 +}$ will reduce $F e^{3 +} to F e^{2 +}$

$C l_{2}$ will be liberated from $K C l$ by passing $I_{2} .$

$C e^{4 +}$ can oxidize $F e^{2 +}$

$F e^{3 +}$ oxidizes $C e^{+ 3}$

answer is B, C.

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$F e^{3 +} + C e^{3 +} \to C e^{4 +} + F e^{2 +} E^{O} < 0 I_{2} + C l^{-} \to C l_{2} + I^{-} E^{O} < 0$

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The values of E0 of some electrode reactions are given below I2 + 2e−→ 2I− E0=0.54 voltsSn+4 + 2e−→ Sn2+ E0= 0.152 voltsCl2 + 2e− → 2Cl− E0= 1.36 voltsFe+3 + e− →Fe2+ E0= 0.76 voltsCe+4 + e− → Ce3+ E0= 1.6 voltsChoose the correct statement(s)

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