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In: Chemistry

Use tabulated electrode potentials to calculate ΔG∘ for the reaction 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq)

Use tabulated electrode potentials to calculate ΔG∘ for the reaction 2K(s)+2H₂O(l)→H₂(g)+2OH⁻(aq)+2K⁺(aq)

Expert Solution

2K(s)+2H₂O(l) → H₂(g)+2OH⁻(aq)+2K⁺(aq)

The oxidation half cell reaction is : K(s) → K⁺(aq) + e^- ; E^o_K+/K = -2.925 V ---(1)

The reduction half cell reaction is : 2H₂O(l) + 2 e^- → H₂(g)+2OH^-(aq) ; E^o_2H+/H2 = -0.8277V ---(2)

Overall reaction is obtained as follows : [2xEqn(1)] + [Eqn(2)]

So standard potential of the cell , E^o = E^o_cathode - E^o_anode

= E^o_2H+/H2- E^o_K+/K

= -0.8277 - (-2.925) V

= +2.0973 V

We know that G^o = -nFE^o

Where

n = number of electrons transferred = 2

F = faraday = 96500 C

Plug the values we get G^o = -nFE^o

= -(2x96500x2.0973)

= -404.8x10³ J

= - 404.8 kJ

Therefore G^o = - 404.8 kJ

queen_honey_blossom answered 11 months ago

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