The standard reduction potentials of the following half-reactions are given in Appendix E in the textbook:
Ag+(aq)+e−→Ag(s)= .799
Cu2+(aq)+2e−→Cu(s)= .337
Ni2+(aq)+2e−→Ni(s)= -.28
Cr3+(aq)+3e−→Cr(s). = -.74
1. Determine which combination of these half-cell reactions leads to the cell reaction with the largest positive cell emf.
1st and 2nd, |
1st and 3rd, |
1st and 4th, |
2nd and 3rd, |
3rd and 4th. |
It isn't the first or last one because I have gotten it wrong twice.
2. Calculate the value of this emf.
3. Then determine which combination is the smallest and calculate the emf.
1] Ag+(aq)+e−→Ag(s)= 0.799
Cr3+(aq)+3e−→Cr(s). = -0.74
The combination 1st and 4th cell provides large psoitive emf
2] 3Ag+ + Cr -----> 3Ag + Cr+3
The emf of the reaction is 0.799+0.74 = 1.539 V
3] 3rd and 4th combination gives small postive emf
Ni2+(aq)+2e−→Ni(s)
Cr3+(aq)+3e−→Cr(s)
----------------------------------
3Ni+2 + 2Cr------> 3Ni + 2Cr+3
Emf = 0.74 - 0.28 = 0.46 V
The standard reduction potentials of the following half-reactions are given in Appendix E in the textbook:...
Use the standard reduction potentials from the following table to choose the weakest reducing agent among those shown below. Ag+(aq) + - + Ag(s) E° = 0.80 V Cu2+(aq) + 2e → Cu(s) E° = 0.34 V Ni2+(aq) + 2e + Ni(s) E° = -0.26 V Cr3+(aq) + 3e- → Cr(s) E° = -0.74 V Mn2+(aq) + 2e → Mn(s) E° = -1.19 V О Ni(s) Ag(s) Cr(s) Mn(s) Cu(s)
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