1
JEE Main 2019 (Online) 9th April Evening Slot
+4
-1
A solution of Ni(NO3)2 is electrolysed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni will be deposited at the cathode?
A
0.10
B
0.15
C
0.20
D
0.05
2
JEE Main 2019 (Online) 9th April Morning Slot
+4
-1
The standard Gibbs energy for the given cell reaction in kJ mol–1 at 298 K is :

Zn(s) + Cu2+ (aq) $$\to$$ Zn2+ (aq) + Cu (s),

E° = 2 V at 298 K

(Faraday's constant, F = 96000 C mol–1)
A
384
B
–192
C
–384
D
192
3
JEE Main 2019 (Online) 8th April Evening Slot
+4
-1
Calculate the standard cell potential in (V) of the cell in which following reaction takes place :

Fe2+(aq) + Ag+(aq) $$\to$$ Fe3+(aq) + Ag (s)

Given that

$$E_{A{g^ + }/Ag}^o = xV$$

$$E_{Fe^{2+ }/Fe}^o = yV$$

$$E_{Fe^{3+ }/Fe}^o = zV$$
A
x + 2y - 3z
B
x - z
C
x - y
D
x + y - z
4
JEE Main 2019 (Online) 8th April Morning Slot
+4
-1
Given that $${E^\Theta }_{{O_2}/{H_2}O} = 1.23\,V$$ ;

$${E^\Theta }_{{S_2}O_8^{2 - }/SO_4^{2 - }} = 2.05\,V$$

$${E^\Theta }_{B{r_2}/B{r^ - }} = 1.09\,V$$

$${E^\Theta }_{A{u^{3 + }}/Au} = 1.4\,V$$

The strongest oxidizing agent is :
A
O2
B
Au3+
C
Br2
D
$${S_2}O_8^{2 - }$$
EXAM MAP
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