Relative Half-Cell Potentials Assuming standard conditions, answer the following
ID: 559703 • Letter: R
Question
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!
Explanation / Answer
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