The number of Faradays(F) required to produce 20 g of calcium from molten CaCl2 (Atomic mass of Ca = 40 g mol-1) is :
A
2
B
3
C
4
D
1
2
NEET 2019
MCQ (Single Correct Answer)
+4
-1
For a cell involving one electron $$E_{cell}^\Theta $$ = 0.59 V at 298 K, the equilibrium constant for the cell reaction is :
[Given that $${{2.303RT} \over F}$$ = 0.059 V at T = 298 K ]
A
1.0 $$ \times $$ 1030
B
1.0 $$ \times $$ 1010
C
1.0 $$ \times $$ 102
D
1.0 $$ \times $$ 105
3
NEET 2019
MCQ (Single Correct Answer)
+4
-1
For the cell reaction
2Fe3+(aq) + 2I–
(aq) $$ \to $$ 2Fe2+(aq) + I2(aq)
$${E_{cell}^\Theta }$$ = 0.24 V at 298 K. The standard Gibbs energy ($$\Delta $$rGo) of the cell reaction is :
[Given that Faraday constant F = 96500 C mol–1]
A
46.32 kJ mol–1
B
23.16 kJ mol–1
C
–46.32 kJ mol–1
D
–23.16 kJ mol–1
4
NEET 2018
MCQ (Single Correct Answer)
+4
-1
Consider the change in oxidation state of
bromine corresponding to different emf values
as shown in the given diagram :
Then the species undergoing disproportionation
is :
