If a strip of Ni were dipped into a solution of AgNO3, what wuold be expected to occur

If a strip of Ni were dipped into a solution of AgNO3, what wuold be expected to occur? Explain, using E^0 values.

we expect that Ni will oxidize to Ni+2
while Ag+ is reduced to Ag metal

from
http://bilbo.chm.uri.edu/CHM112/tables/r…
standard reduction: Ag+(aq) + 1 e- --> Ag(s) E^o = + 0.800 volts
we see that Ag+ from the AgNO3 has a strong pull for electrons

standard reduction: Ni2+(aq) + 2 e- --> Ni(s) E^o = – 0.257 volts
we see that NI+2 does not have a strong pull for electrons
but rather the reverse reaction is more likely:
oxidation: Ni(s) --> Ni2+(aq) + 2 e- E^o = + 0.257 volts


we get a redox reaction,
reduction: Ag+(aq) + 1 e- --> Ag(s) E^o = + 0.800 volts
oxidation: Ni(s) --> Ni2+(aq) + 2 e- E^o = + 0.257 volts
where Ag+ ions spontaneously takes electrons,
while Ni metal spontaneously loses electrons


Ni (s) & 2AgNO3 (aq) --> 2 Ag (s) & Ni(NO3)2 (aq)