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Write the half reaction for the reaction...

Write the half reaction for the reaction
`2Fe^(+3) + 2I^(-) to 2Fe^(+2) + I_(2)`

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To write the half-reactions for the given redox reaction \(2Fe^{3+} + 2I^{-} \rightarrow 2Fe^{2+} + I_{2}\), we need to identify the oxidation and reduction processes occurring in the reaction. ### Step-by-Step Solution: 1. **Identify Oxidation and Reduction:** - In the reaction, iron (\(Fe\)) is reduced from \(Fe^{3+}\) to \(Fe^{2+}\). - Iodide ion (\(I^{-}\)) is oxidized to iodine (\(I_{2}\)). ...
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Standard reduction potential of I_(3)^(-), I^(-) and Fe^(3+), Fe^(2+) are 0.54 and 0.77 V , respectively . Calculate the equilibrium constant for the reaction. 2Fe^(3+) + 3I^(-)

Given electrode potentials: Fe^(3+) + e^(-) rarr Fe^(2+) : E^(o) =0.771 V and I_(2) 2e^(-) rarr 2I^(-), E^(o) = 0.556 V then E^(o) for the cell reaction 2 Fe^(3+) 2I ^(-) rarr 2 Fe^(2+) + l_(2) will be:

Knowledge Check

  • Calculate the euilibrium constant for the reaction, 2Fe^(3+) + 3I^(-) hArr 2Fe^(2+) + I_(3)^(-) . The standard reduction potential in acidic conditions are 0.77 V and 0.54 V respectivelu for Fe^(3+)//Fe^(2+) and I_(3)^(-)//I^(-) couples.

    A
    `4.25xx10^7`
    B
    `7.05xx10^5`
    C
    `6.25xx10^5`
    D
    `6.25xx10^7`

  • The cell in which the following reaction occurs : 2Fe_(aq)^(3+) + 2I_(aq)^(-) to 2Fe_(aq)^(2+) + I_(2(s)) "has" E_("cell")^(o) = 0.236 V "at" 298 K The equilibrium constnat of the cell reaction is

    A
    `6.69xx 10^(-7)`
    B
    `9.69 xx 10^(-7)`
    C
    `9.69 xx 10^(7)`
    D
    `6.69 xx 10^(7)`

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    Consider the following reactions. DeltaH^(@) values of the reactions hve been given as -x, -y and z kJ. Fe_(3)O_(4)(s) to 3Fe(s) + 2O_(2)(g), DeltaH^(@) = z kJ 2Fe(s) + O_(2)(g) to 2FeO(s), DeltaH^(@) =-x kJ 4Fe(s) + 3O_(2)(g) to 2Fe_(2)O_(3)(s), DeltaH^(@) =-y kJ Heat of reaction for the reaction, FeO(s) + Fe_(2)O_(3)(s) to Fe_(3)O_(4)(s) is :

    Consider the following E^(@) values E^(@) values E_(Fe^(3+)//Fe^(2+))^(@)= 0.77v , E_(Sn^(2+)//Sn)^(@) = -0.14 under standard condition the potential for the reaction Sn_(s)+ 2Fe^(3+)(aq)rightarrow 2Fe^(2+)(aq) + Sn^(2+) (aq) is :

    The half cell reactions for rusting of iron are : 2H^(+) + 2e^(-) + (1)/(2)O_(2) rightarrow H_(2)O (l) , E^(@) = +1.23V Fe^(2+) + 2e^(-) rightarrow Fe , E^(@) = -0.44V Delta^(@) ((inKJ) for the reaction is : Fe+2H^(+) + (1)/(2) O_(2)rightarrow Fe^(+2)+ H_(2) O ((l))

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    N-factor for the following reaction is FeS_(2)toFe_(2)O_(3)+SO_(2)

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