1
JEE Main 2019 (Online) 10th January Evening Slot
+4
-1
In the cell

Pt$$\left| {\left( s \right)} \right|$$H2(g, 1 bar)$$\left| {HCl\left( {aq} \right)} \right|$$AgCl$$\left| {\left( s \right)} \right|$$Ag(s)|Pt(s)

the cell potential is 0.92 V when a 10–6 molal HCl solution is used. The standard electrode potential of (AgCl/ AgCl ) electrode is :
$$\left\{ {} \right.$$Given,  $${{2.303RT} \over F} = 0.06V$$  at  $$\left. {298} \right\}$$
A
0.94 V
B
0.40 V
C
0.76 V
D
0.20 V
2
JEE Main 2019 (Online) 10th January Morning Slot
+4
-1
Consider the following reduction processes :
Zn2+ + 2e $$\to$$ Zn(s) ; Eo = – 0.76 V
Ca2+ + 2e $$\to$$ Ca(s); Eo = –2.87 V
Mg2+ + 2e $$\to$$ Mg(s) ; Eo = – 2.36 V
Ni2 + 2e $$\to$$ Ni(s) ; Eo = – 0.25
The reducing power of the metals increases in the order :
A
Ca < Mg < Zn < Ni
B
Ni < Zn < Mg < Ca
C
Zn < Mg < Ni < Ca
D
Ca < Zn < Mg < Ni
3
JEE Main 2019 (Online) 9th January Evening Slot
+4
-1
If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction

Zn(s) + Cu2+ (aq) $$\rightleftharpoons$$ Zn2+(aq) + Cu(s)

at 300 K is approximately,

(R = 8 JK$$-$$1mol$$-$$1, F = 96000 C mol$$-$$1)
A
e$$-$$80
B
e$$-$$160
C
e320
D
e160
4
JEE Main 2019 (Online) 9th January Morning Slot
+4
-1
The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO4 electrolyzed in g during the process is : (Molar mass of PbSO4 = 303 g mol$$-$$1)
A
22.8
B
15.2
C
7.6
D
11.4
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