Calulate E naught cell for the reaction below
5 Cd(s) + 2 MnO4^-(aq) + 16H+(aq)+ 2 Mn2+(aq) + 8 HxsO(l)
The oxidation anode must be 5Cd(s) ==> 5Cd2+(aq) +10e^-
The reduction cathode must be 2MnO4^- + 16H2^=(aq) + 10e^- ==> 2Mn2+(aq) + 8H2O
E naught cell = E naught cathode - E naught anode = (+1.52V) - (-0.40V) = +1.92V
I agree with 1.92 v.
To calculate the standard cell potential (E naught cell) for the given reaction, you need to find the standard reduction potentials of the cathode and the anode.
1. Start by writing the oxidation half-reaction, which is the anode:
5 Cd(s) → 5 Cd2+(aq) + 10 e^-
2. Look up the standard reduction potential for the Cd2+/Cd half-reaction. The value is -0.40 V (given).
3. Write the reduction half-reaction, which is the cathode:
2 MnO4^-(aq) + 16 H+(aq) + 10 e^- → 2 Mn2+(aq) + 8 H2O
4. Look up the standard reduction potential for the MnO4^-/Mn2+ half-reaction. The value is +1.52 V (given).
5. Subtract the standard reduction potential of the anode (Cd2+/Cd) from the standard reduction potential of the cathode (MnO4^-/Mn2+):
E naught cell = E naught cathode - E naught anode = (+1.52 V) - (-0.40 V) = +1.92 V
Therefore, the standard cell potential (E naught cell) for the given reaction is +1.92 V.
To calculate the standard cell potential, E naught cell, for the given redox reaction, you need to know the standard reduction potentials for both the oxidation reaction at the anode and the reduction reaction at the cathode.
First, let's identify the half-reactions involved in the reaction:
Oxidation at the anode:
5 Cd(s) → 5 Cd2+(aq) + 10 e-
Reduction at the cathode:
2 MnO4-(aq) + 16 H+(aq) + 10 e- → 2 Mn2+(aq) + 8 H2O(l)
Next, look up the standard reduction potentials, E naught, for each half-reaction. The reduction potential can be found in reference tables or online databases. For example, E naught for the Cd2+/Cd half-reaction is -0.40V, and E naught for the MnO4-/Mn2+ half-reaction is +1.52V.
To calculate E naught cell, subtract the E naught of the anode reaction from the E naught of the cathode reaction:
E naught cell = E naught cathode - E naught anode
E naught cell = (+1.52V) - (-0.40V)
E naught cell = +1.92V
Therefore, the standard cell potential, E naught cell, for the given reaction is +1.92V.