a) Calculate the cell potential at 25°C for the cell Fe(s) I (Fe2+ (0.100 M) II...

a) Calculate the cell potential at 25°C for the cell

Fe(s) I (Fe²⁺ (0.100 M) II Pd²⁺ (1.0 × 10^-5 M) I Pd(s)

given that the standard reduction potential for Fe²⁺/Fe is -0.45 V and for Pd²⁺/Pd is +0.95 V. - Please show the steps

b) Based on the half-reactions and their respective standard reduction potentials below, the strongest reducing agent is ________, and the strongest oxidizing agent is ________.

Ag⁺ (aq) + e^- → Ag(s) 0.80 V

2 H⁺ (aq) + 2 e^- → H₂ (g) 0.00 V

Cd²⁺ (aq) + 2 e^- → Cd(s) -0.40 V

The answer is

Cd, Ag⁺

Can you please explain to me why this is the right answer.

Solutions

Expert Solution

queen_honey_blossom answered 8 months ago

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