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If Fe is allowed to react with 1(M) HCl ...

If `Fe` is allowed to react with 1(M) HCl solution, will Fe be oxidised to `Fe^(2+)? E_(Fe^(+2)|Fe)^(@)=-0.44V`

Text Solution

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If `Fe` reacts with `HCl,` then it will get oxidised to `Fe^(2+)`
`Fe(s)rarr Fe^(2+)(aq)+2e, E_("anode")^(@)=-0.44V`
`and H^(+)(aq)` will be reduced to `H_(2)(g)` is
`2H^(+)(aq)+2e rarr H_(2)(g), E_("anode")^(@)=0.00V`
`"Net reaction :Fe(s)+2H^(+)(aq)rarr Fe^(2+)(aq)+H_(2)(g)`
`E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)=[0.00-(-0.44)]=+0.44V`
Since `E_("cell")^(@)gt0`, the reaction (1) will occur spontaneously at standard conditions. Hence, Fe will reduce `H^(+)(aq)` ions to `H_(2)(g),` and it will itself get oxidised to `Fe^(2+)`.
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Knowledge Check

  • A solution contains Fe^(3+), Fe^(2+) and I^(-) ions. This solution was treated with iodine at 35^(@)C . E_(Fe^(3+)|Fe^(2+))^(@)=+0.77V and E_(I_(2)|2I^(-))^(@)=+-.536V . The favourable redox reaction is -

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  • The standard free energy of the reaction Fe(s)+Sn^(2+)(aq, 1M)rarr Fe^(2+)(aq, 1M)+Sn(s) is ("given : at "25^(@)C, E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Sn^(2+)|Sn)^(@)=-0.14V)-

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