1
IIT-JEE 1997
Subjective
+2
-0
Calculate the equilibrium constant for the reaction
Fe2+ + Ce4+ $$\leftrightharpoons$$ Fe3+ + Ce3+
(given $$E_{C{e^{4 + }}/C{e^{3 + }}}^o$$ = 1.44 V; $$E_{F{e^{3 + }}/F{e^{2 + }}}^o$$ = 0.68 V)
2
IIT-JEE 1996
Subjective
+3
-0
The standard reduction potential for Cu2+|Cu is +0.34 V. Calculate the reduction potential at pH = 14 for the above couple. Ksp of Cu(OH)2 is 1.0 $$\times$$ 10-19
3
IIT-JEE 1995
Subjective
+4
-0
An excess of liquid mercury is added to an acidified solution of 1.0 $$\times$$ 10-3 M Fe3+. It is found that 5% of Fe3+ remains at equilibrium at 25oC. Calculate $$E_{Hg_2^{2 + }|\,Hg}^o$$, assuming that only reaction that occurs is
2Hg + 2Fe3+ $$\to$$ $$Hg_2^{2+}$$ + 2Fe2+
(Given $$E_{F{e^{3 + }}|\,F{e^{2 + }}}^o$$ = 0.77 V)
4
IIT-JEE 1994
Subjective
+4
-0
The Edison storage cells is represented as
Fe(s) | FeO(s) | KOH (aq) | Ni2O3(s) | Ni(s)
The half-cell reactions are:
Ni2O3 + H2O (l) + 2e- $$\leftrightharpoons$$ 2NiO(s) + 2OH-; Eo = +0.40V
FeO(s) + H2O(l) + 2e- $$\leftrightharpoons$$ Fe(s) + 2OH-; Eo = -0.87V
(i) What is the cell reaction?
(ii) What is the cell e.m.f? How does it depend on the concentration of KOH?
(iii) What is the maximum amount of electrical energy that can be obtained from one mole of Ni2O3?
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