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Two half-reactions of an electrochemical...

Two half-reactions of an electrochemical cell are given below:
`MnO_(4)^(-)(aq) +8H^(+) (aq) +5e^(-) to Mn^(2+)(aq) +4H_(2)O(l), E^(Theta)= +1.51V`
`Sn^(2+)(aq) to Sn^(4+)(aq)+2e^(-), E^(Theta)=0.15V`
Construct the redox reaction equation from the two half reactions and calculate the cell potential from the standard potentials and predict if the reaction is reactant or product favoured.

Text Solution

Verified by Experts

At anode : `Sn_((aq))^(2+)rightarrow Sn_((aq))^(4+) + 2e^(-) ]xx5`
At cathode : `MnO_(4)^(-) (aq) + 8H_((aq))^(+) + 5e^(-)rightarrow Mn_((aq))^(2+) + 4H_(2)O_((1))]xx2`
Net cell reaction : `2MnO_(4) ^(-) + 5Sn_((aq))^(2+) + 16H_((aq))^(+)rightarrow2Mn_((aq))^(2+) + 5Sn_((aq))^(4+)+ 8H_(2)O_((1))`
`E_(cell)^(@) = E_(cathode)^(@) -E_(anode)^(@) = 1.51V - 0.15V - 0.15V = 1.36V`
Since, cell potential is positive therefore the reaction is product favoured.
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Two half cell reactions of an electrochemical cell are given below : MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-),toMn^(2+)(aq)+4H_(2)O(l),E^(@)=+1.51V Sn^(2+)(aq)toSn^(4+)(aq)+2e^(-),E^(@)=+0.51V Construct the redox equation from the two half cell reactions and predict if the reaction favours formation of reactant or product shown in the equation.

MnO_(4)^(-) + 8H^(+) + 5e^(-) rightarrow Mn^(2+) + 4H_(2)O , E^(@) = 1.51V MnO_(2) + 4H^(+) + 2e^(-) righarrow Mn^(2+) + 2H_(2)O E^(@) = 1.23V E_(MnO_(4)^(-)|MnO_(2)

Knowledge Check

  • Which of the following expression is correct for the rate of reaction given below ? 5Br^(-)(aq) + BrO_(3)^(-)(aq) + 6H^(+) (aq) to 3Br_(2) (aq) + 3H_(2) O(l) .

    A
    `(Delta[Br^(-)])/(Delta t) = 5 (Delta[H^(+)])/(Delta)`
    B
    `(Delta[Br^(-)])/(Delta t) = (6)/(5) (Delta[H^(+)])/(Delta t)`
    C
    `(Delta[Br^(-)])/(Delta t) = (5)/(6) (Delta [H^(+)])/(Delta t)`
    D
    `(Delta[Br^(-)])/(Delta t) = 6 (Delta[H^(+)])/(Delta t)`

  • Which of the following expressions is correct for the rate of reaction given below? 5 Br^(-) (aq) +BrO_(3)^(-) (aq) + 6H^(+) (aq) to 3Br_2(aq) + 2H_2 O(l)

    A
    `(Delta [Br^(-)])/(Delta t)=5 ( Delta [H^(+)])/( Delta t)`
    B
    `(Delta [Br^(-)])/(Delta t)=6/5 ( Delta [H^(+)])/( Delta t)`
    C
    `(Delta [Br^(-)])/(Delta t)=5/6 ( Delta [H^(+)])/( Delta t)`
    D
    `(Delta [Br^(-)])/(Delta t)=6 ( Delta [H^(+)])/( Delta t)`

  • Which of the following expressions is correct for the rate of reaction given below? 5 Br^(-) (aq) +BrO_(3)^(-) (aq) + 6H^(+) (aq) to 3Br_2(aq) + 2H_2 O(l)

    A
    `(Delta [Br^(-)])/(Delta t)=5 ( Delta [H^(+)])/( Delta t)`
    B
    `(Delta [Br^(-)])/(Delta t)=6/5 ( Delta [H^(+)])/( Delta t)`
    C
    `(Delta [Br^(-)])/(Delta t)=5/6 ( Delta [H^(+)])/( Delta t)`
    D
    `(Delta [Br^(-)])/(Delta t)=6 ( Delta [H^(+)])/( Delta t)`

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