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Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction...

Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) cf Table 11.1 on p 403 of Zumdahl 8th ed.

Is Sn2+(aq) capable of oxidizing Fe2+(aq)?

Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)?

Is Ni2+(aq) capable of oxidizing H2(g)?

Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)?

Is Fe2+(aq) capable of oxidizing Cr metal?

Is Fe2+(aq) capable of reducing VO2+(aq)?

Please help and also would like an explanation on how to do this!

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Answer #1

Sn+2 + 2e- ====== Sn(s) E = -0.14

Fe+3 + e- ======= Fe+2 E = 0.771

Th+ Fe has a higher E value in the chart than the Sn so The Fe will oxidize the Sn+2 m answer is No, The Sn will reduce the Fe

b) Cr+3 + e ==== Cr+2 E = -0.41 V

Fe+3 + e- ====== Fe+2 E = 0.771 V

From this potential standards we can see that the Cr will oxidize and that the Fe will reduce , the Fe has more oxidating power.

Answer is No the Cr+3 will not oxidize the Fe+3

c) Ni + 2e ===Ni+2 E = -0.25 V

2H + 2e === H2 E = 0 V

Nickel is the reducing agent so the answer is No, the Nickel will not oxidize the hydrogen

d) Sn+2 + 2e ====== Sn (s) E = -0.14 V

Fe+3 + e- ====== Fe+2 E = 0.771 V

Fe+3 is the oxidating agent because it has a higher value of E so

Sn metal will be oxidized and Fe+3 will be reduced so this is TRUE

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