1
IIT-JEE 2005
Subjective
+6
-0
(a). For the reaction
Ag+ (aq) + Cl- (aq) $$\leftrightharpoons$$ AgCl (s)
Given:
Species $$\Delta G_f^o$$ (kJ/mol)
Ag+ (aq) +77
Cl- (aq) -129
AgCl (s) -109

Write the cell representation of above reaction and calculate $$E_{cell}^o$$ at 298 K. Also find the solubility product if AgCl.
(b) If 6.539 $$\times$$ 10-2 g of metallic zinc is added to 100 ml saturated solution of AgCl. Find the value of $${\log _{10}}{{\left[ {Z{n^{2 + }}} \right]} \over {{{\left[ {A{g^ + }} \right]}^2}}}$$. How many moles of Ag will be precipitated in the above reaction. Given that
Ag+ + e- $$\to$$ Ag; Eo = 0.80 V;
Zn2+ + 2e- $$\to$$ Zn; Eo = -0.76 V;
(It was given that atomic mass of Zn = 65.39)
2
IIT-JEE 2004
Subjective
+4
-0
Find the equilibrium constant for the reaction,
In2+ + Cu2+ $$\to$$ In3+ + Cu+ at 298 K
given
$$E_{C{u^{2 + }}/C{u^ + }}^o$$ = 0.15 V; $$E_{l{n^{2 + }}/l{n^ + }}^o$$ = -0.40 V; $$E_{l{n^{3 + }}/l{n^ + }}^o$$ = -0.42 V;
3
IIT-JEE 2003
Subjective
+2
-0
Two students use the same stock solution of ZnSO4 and solution of CuSO4. The emf of one cell is 0.03 V higher than other. The conc. of CuSO4 in the cell with higher emf value is 0.5 M. Find out the conc. of CuSO4 in the other cell (2.203 RT/F = 0.06)
4
IIT-JEE 2001
Subjective
+10
-0
The standard potential of the following cell is 0.23V at 15oC and 0.21 V at 35oC.
Pt | H2 (g) | HCl (aq) | AgCl (s) | Ag (s)
(i) Write the cell reaction.
(ii) Calculate $$\Delta H^o$$ and $$\Delta S^o$$m for the cell reaction by assuming that these quantities remain unchanged in the range 15oC to 35oC.
(iii) Calculate the solubility of AgCl in water at 25oC
Given : The standard reduction potential of the Ag+ (aq) / Ag (s) couple is 0.80 V at 25oC
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