1

IIT-JEE 2005

Subjective

+6

-0

(a). For the reaction

Ag

Given:

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

Ag

Zn

(It was given that atomic mass of Zn = 65.39)

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 thatAg

^{+}+ e^{-}$$\to$$ Ag; E^{o}= 0.80 V;Zn

^{2+}+ 2e^{-}$$\to$$ Zn; E^{o}= -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,

In

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;

In

^{2+}+ Cu^{2+}$$\to$$ In^{3+}+ Cu^{+}at 298 Kgiven

$$E_{C{u^{2 + }}/C{u^ + }}^o$$ = 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 ZnSO

_{4}and solution of CuSO_{4}. The emf of one cell is 0.03 V higher than other. The conc. of CuSO_{4}in the cell with higher emf value is 0.5 M. Find out the conc. of CuSO_{4}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 15

Pt | H

(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 15

(iii) Calculate the solubility of AgCl in water at 25

^{o}C and 0.21 V at 35^{o}C.Pt | H

_{2}(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 15

^{o}C to 35^{o}C.(iii) Calculate the solubility of AgCl in water at 25

^{o}C**Given :**The standard reduction potential of the Ag^{+}(aq) / Ag (s) couple is 0.80 V at 25^{o}CQuestions Asked from Electrochemistry (Subjective)

Number in Brackets after Paper Indicates No. of Questions

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