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When answering Parts a-h, consider only the molecules and ions, Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq),

and Cr2O7^2-(aq), under standard state conditions. (1 pt each) Use standard reduction table.

a) Which of these molecules and ions are oxidizing agents?

b) Which of these molecules and ions are reducing agents?

c) List the oxidizing agents from part a in DECREASING order of oxidizing agent strength. (strongest OA to weakest OA)

d) List the reducing agents from part b in DECREASING order of reducing agent strength. (strongest RA to weakest RA)

e) Fe2+(aq) can be an oxidizing agent and a reducing agent.
i) Write the half-reaction where Fe2+(aq) is the oxidizing agent.

ii) Write the half-reaction where Fe2+(aq) is the reducing agent.
f) Which of these molecules and ions can be oxidized by Fe2+?
g) Write a balanced spontaneous redox reaction where one of these molecules or ions is oxidized by Fe2+.

h) Which of these molecules and ions can be reduced by Fe2+?
Standard Reduction Table at 25 C Redox Couple Half-Reaction 2.87 MnOd +4 H+ + 3 e. → MnO2+ 2H2O 1.68 Mn 1.50 Ch+2e-20 1.36 1.

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When answering Parts a-h, consider only the molecules and ions, Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq), and Cr2O7^2-(aq), under standard state conditions. (1 pt each) Use standard reduction...
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