A strip of nickel metal is dipped in a 1 molar solution of `Ni (NO_(3))_(2)` and a strip of silver metal is dipped in a 1 molar solution of `AgNO_(3)`. An electrochemical cell is created when the two solutions are joined by salt bridge and two strips are joined by wire to a voltmeter.
Answer the following questions.
Write the balanced equation for the overall cell reaction and calculate the cell potential.

Explanation

The half-cell reaction
At anode, `Ni(s) to Ni^(2+) (1M) +2e^(-)`
At cathode,
`2Ag^(+) (1M)+2e^(-) to 2Ag(s)`
Overall reaction, `Ni+2Ag^(+) to Ni^(2+) +2Ag`
Number of electrons, (n) = 2
`E_("cell")^(@) =E_("cathode")^(@) -E_("anode")^(@) = 0.80 -(-0.25)`
`E_("cell")^(@)=1.05V`
By using Nernst equation,
`E_("cell")=E_("cell")^(@)-(0.0591)/(n)"log" ([Ni^(2+)])/([Ag^(+)]^(2))`
`E_("cell")=1.05 -(0.05 91)/(2) log (1) =1.05 -(0.0591)/(2) xx 0`
`E_("cell")=1.05V`