Description

The chemistry of electrochemical cells involves redox reactions. In this assignment, demonstrate your understanding of the electrode potential and half reactions by completing a problem set.

Instructions

Your task is to complete the questions in the problem set. Please note that you must include units throughout all of your calculations and provide your answer in scientific notation to the correct number of significant digits.

Questions

For each of the cell diagrams, provide the following information:

the 

  1. The two redox half reactions (oxidation and reduction) (1 marks each)

The balanced net ionic equation (1 mark each)

  • Whether the reaction is spontaneous 
  • 2. Is this cell equation correct? Explain and justify your answer
  • A table containing the standard reduction potentials at 25 oC is provided.

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UNFORMATTED ATTACHMENT PREVIEW

Standard Reduction Potentials at 25ºC E° (V) Reduction Half-Reaction F₂(g) + 2 e− 2 F (aq) 2.87 H₂O₂(aq) + 2 H⁺(aq) + 2 e− 2 H₂O(l) 1.78 MnO₄−(aq) + 8 H⁺(aq) + 5 e− Mn2+(aq) + 4 H₂O(l) 1.51 Cl₂(g) + 2 e− 2 Cl−(aq) 1.36 Cr₂O₇2−(aq) + 14 H⁺(aq) + 6 e− 2 Cr3+(aq) + 7 H₂O(l) 1.33 O₂(g) + 4 H⁺(aq) + 4 e− 2 H₂O(l) 1.23 Br₂(l) + 2 e− 2 Br−(aq) 1.09 Ag⁺(aq) + e− Ag(s) 0.80 Fe3⁺(aq) + e− Fe2+(aq) 0.77 O₂(g) + 2 H⁺(aq) + 2 e− H₂O₂(aq) 0.70 I₂(s) + 2 e− 2 I−(aq) 0.54 O₂(g) + 2 H₂O(l) + 4 e− 4 OH−(aq) 0.40 Cu2⁺(aq) + 2 e− Cu(s) 0.34 Sn4⁺(aq) + 2 e− Sn2+(aq) 0.15 2 H⁺(aq) + 2 e− H₂(g) 0 Pb2⁺(aq) + 2 e− Pb(s) ‒0.13 Ni2⁺(aq) + 2 e− Ni(s) ‒0.26 Cd2⁺(aq) + 2 e− Cd(s) ‒0.40 Fe2⁺(aq) + 2 e− Fe(s) ‒0.45 Zn2⁺(aq) + 2 e− Zn(s) ‒0.76 2 H₂O(l) + 2 e− H₂(g) + 2 OH−(aq) ‒0.83 Al3⁺(aq) + 3 e− Al(s) ‒1.66 Mg2⁺(aq) + 2 e− Mg(s) ‒2.37 Na⁺(aq) + e− Na(s) ‒2.71 Li⁺(aq) + e−

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