Chemistry: The overall reaction 2co3+(aq) + 2cl–(aq) → 2co2+(aq) + cl2(g) has the standard cell voltage e°cell = 0.46 v. given e° = 1.36 v for the reaction cl2(g) + 2e– → 2cl–(aq), calculate the standard reduction potential for the following the half reaction at 25°c: co3+ + e– → co2+

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The overall reaction 2co3+(aq) + 2cl–(aq) → 2co2+(aq) - id232224048591, deonnaturner68p7hz7y

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14.02.2022

The standard reduction potential for reduction half reaction is 1.82 V

Explanation:

The given chemical reaction follows:

$2Co^{3+}(aq.)+2Cl^(aq.)\rightarrow 2Co^{2+}(aq.)+Cl_2(g)$

Oxidation half reaction: $2Cl^-\rightarrow Cl_2+2e^-$

Reduction half reaction: $Co^{3+}+e^-\rightarrow Co^{2+}$

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

We are given:

$E^o_{Cl_2/2Cl^-}=1.36V\\\\E^o_{cell}=0.46V$

Putting values in above equation, we get:

$0.46=E^o_{Co^{3+}/Co^{2+}}-1.36\\\\E^o_{Co^{3+}/Co^{2+}}=(0.46+1.36)V=1.82V$

Hence, the standard reduction potential for reduction half reaction is 1.82 V

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