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The half cell reactions for rusting of i...

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))`

A

`(-76)`

B

`(-322)`

C

`(-122)`

D

`(-176)`

Text Solution

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To find the Gibbs free energy change (ΔG°) for the reaction: \[ \text{Fe} + 2\text{H}^+ + \frac{1}{2}\text{O}_2 \rightarrow \text{Fe}^{2+} + \text{H}_2\text{O} \] we will follow these steps: ### Step 1: Identify the half-cell reactions and their standard potentials The half-cell reactions given are: ...
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The rusting of iron takes place as follows : 2H^(o+)+2e^(-) +(1)/(2)O_(2)rarr H_(2)O(l)," "E^(@)=+1.23V Fe^(2+)+2e^(-) rarr Fe(s)," "E^(@)=-0.44V Calculate DeltaG^(@) for the net process.

The rusting of iron takes place as follows : 2H^(o+)+2e^(-) +(1)/(2)O_(2)rarr H_(2)O(l)," "E^(c-)=+1.23V Fe^(2+)+2e^(-) rarr Fe(s)," "E^(c-)=-0.44V Calculae DeltaG^(c-) for the net process.

The rusting of iron takes place as follows : 2H^(o+)+2e^(-) +(1)/(2)O_(2)rarr H_(2)O(l)," "E^(c-)=+1.23V Fe^(2+)+2e^(-) rarr Fe(s)," "E^(c-)=-0.44V Calculae DeltaG^(c-) for the net process.

The rusting of iron takes place as follows : 2H^(o+)+2e^(-) +(1)/(2)O_(2)rarr H_(2)O(l)," "E^(c-)=+1.23V Fe^(2+)+2e^(-) rarr Fe(s)," "E^(c-)=-0.44V Calculae DeltaG^(c-) for the net process. (a) -322kJ mol^(1) (b) -161kJ mol^(-1) (c) -152kJ mol^(-1) (d) -76kJ mol^(-1)

The standard oxidation potentials, , for the half reactions are as follows : Zn rightarrow Zn^(2+) + 2e^(-) , E^(@) = +0.76V Fe rightarrow Fe^(2+)+ 2e^(-), E^(@) = + 0.41 V The EMF for the cell reaction, Fe^(2+) + Zn rightarrow Zn^(2+) + Fe

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)

In the reactions HCl + NaOH rightarrow NaCl + H_(2)O + x cal. H_(2)SO_(4) + 2NaOH rightarrow Na_(2)SO_(4) + 2 H_(2)O + y cal.

For the reaction C_2H_(5)OH(l) + 3 O_(2)(g) rightarrow 2CO_(2)(g) + 3 H_(2)O(l) , which one is true ?

Potential for some half cell reactions are given below. On the basis of these mark the correct answer. (i) H^(+)(aq) + e^(-) rightarrow (1/2)H^(2)(g) E_(cell)^(@) = 0.00V (ii) 2H_(2)O(l) rightarrow O_(2)(g) + 4H^(+)(aq) + 4e^(-) , E_(cell) = 1.23V (iii) 2SO_(4)^(2-)(aq) rightarrow S_(2)O_(8)^(2-)(aq) + 2e^(-), E_(cell)^(@) = 1.96V

The standard electrode potential of the half cells are given below : Zn^(2+)+ 2e^(-) rarr Zn(s), E^(o) = - 7.62 V Fe^(2+) + 2e^(-) rarr Fe(s) , E^(o) = -7 .81 V The emf of the cell Fe^(2+) + Zn rarr Zn^(2+) + Fe will be :

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