| Reduction half-reaction | E∘ (V) |
| Ag+(aq)+e−→Ag(s) | 0.80 |
| Cu2+(aq)+2e−→Cu(s) | 0.34 |
| Sn4+(aq)+4e−→Sn(s) | 0.15 |
| 2H+(aq)+2e−→H2(g) | 0 |
| Ni2+(aq)+2e−→Ni(s) | −0.26 |
| Fe2+(aq)+2e−→Fe(s) | −0.45 |
| Zn2+(aq)+2e−→Zn(s) | −0.76 |
| Al3+(aq)+3e−→Al(s) | −1.66 |
| Mg2+(aq)+2e−→Mg(s) | −2.37 |
1)
Use the table of standard reduction potentials given above tocalculate the equilibrium constant at standard temperature (25 ∘C)for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)
2)
Calculate the standard cell potential (E∘) for thereaction
X(s)+Y+(aq)→X+(aq)+Y(s)
if K = 3.80×10−4.
Express your answer to three significant figures and include theappropriate units.
