1
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)
2
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?
3
IIT-JEE 1994
Subjective
+3
-0
The standard reduction potential of the Ag+/Ag electrode at 298 K is 0.799V. Given that for AgI, Ksp = 8.7 $$\times$$ 10-17, evaluate the potential of the Ag+/Ag electrode in a saturated solution of AgI. Also calculate the standard reduction potential of the I-/ AgI/Ag electrode.
4
IIT-JEE 1993
Subjective
+2
-0
The standard reduction potential for the half-cell
$$NO_3^-$$ + 2H+ (aq) + e $$\to$$ NO2 (g) + H2O is 0.78 V
(i) Calculate the reduction potential in 8 M H+
(ii) What will be the reduction potential of the half-cell in a neutral solution? Assume all the other species to be at unit concentration.
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