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

Explanation

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+)`.