The 25. reduction potentials for Au3* and Ni2* are as follows:
: +1.50 V
E :4.23 Y
Au
nN +
U- i2* 2e- -+ Ni
R
Aur* + 3e- -+
+
t = t.\-L'o't))
E"
t.Jz",t.
Calculate AGo (at 25'C) for t}re reaction:
3Ni-+ 3Ni2* + 2Au
2Au3* +
b
= -nFE"rd),
D0"
a)-2l40kJ
b) +5.00 x 102 kJ
@t.oo x lo3 kJ
d) +1.00 x l0'kJ
e) -5.00 x 102 kJ
Qlc)-v
: *br lbut5x ,-tl
P'K-Tfr"c
= Jr{ ,9 ul /N.
26. Determine the equilibrium constant at2ioC for the reaction
t--
Zn + Ni?+ -+ Zn2+ + Ni
Zn?+
+
2e-
r@+2e-+
a)4.1 x
103
b) x
c) 9.3 6.4 x
Y: -0.76v
-+@
108
l0{
E:4.23Y
Ni
e,t^= -o-rt -Gt'1b) = o'J]
v
k n Eo
\., = olofl
lnq
I
r^o'-'
@-o " ol these
e) none
27. A concentration cell is constructed using two$! electrodes with Niz* concentrations of 1.0 M and 1.00 x
iq the two half-cells. The reduction potential ofNi2* is -{.23 V. Calculate the potential of the cell at25"C.
trSo.r
ra
v
Yl.ifl}
v
d) +0.132
e) +0.0592
V
,' 'i-l
Ni't t
:e *> ui
Ed= -e'>3
f = " -
V
o'o}?
l0{
M
Q-o-"
'q?E
= =zz1
o.
6
-+