The electrode potentials of half-cell reactions are: Zn â Zn2+ + 2e- ; E = -0.76 V and Fe â Fe2+ + 2e- ;E = 0.41 V. The e.m.f of cell Fe2+ + Zn âZn2+ + Fe is
+ 1.17 V
- 1.17 V
- 0.35 V
The e.m.f of a galvanic cell with electrode potentials of Al equal to -1.66 V and that of Mg equal to -0.54 V is
+0.44 V
+ 1.12 V
- 0.44 V
-1.12 V
Which of the following element shows maximum number of oxidation states in its compounds?
Eu
La
Gd
Np
Which of the following metal has the highest tendency for the half-cell reaction?
sodium
lithium
potassium
cesium
In the cell reaction Zn | Zn2+ (1M) II CO3+ (1M) | CO2+ (1M), the value of Eocell is (EoZn2+|Zn = -0.76, Eo CO3+|CO3+ = 1.82 V)
2.58 V
3.58 V
4.58 V
5.58 V
In a Daniell cell, the value of standard free energy (ΔGº) is -212.3 kJ at 25ºC. What will be the value of ln Kc?
65.7
85.7
171.7
343.7
The oxidation number of chromium in potassium dichromate is
+ 2
- 2
- 5
+ 6
A Daniell cell is represented as Zn(s) + Cu2+(aq) →ºCu(s) + Zn2+(aq). The value of standard free energy change in the cell is (Eºcell = 1.1V),
300 kJ
-300 kJ
212.3 kJ
-212.3 kJ
Which of the following transition metal shows highest oxidation state?
Sc
Ti
Os
Zn
The amount of mercury deposited by passing 300 C of charge through mercurous sulphate solution is (Take atomic weight of mercury as 200)
0.2 g
0.4 g
0.6 g
0.8 g
