1
JEE Advanced 2024 Paper 2 Online
MCQ (More than One Correct Answer)
+4
-2
Change Language

An aqueous solution of hydrazine $\left(\mathrm{N}_2 \mathrm{H}_4\right)$ is electrochemically oxidized by $\mathrm{O}_2$, thereby releasing chemical energy in the form of electrical energy. One of the products generated from the electrochemical reaction is $\mathrm{N}_2(\mathrm{~g})$.

Choose the correct statement(s) about the above process

A
$\mathrm{OH}^{-}$ions react with $\mathrm{N}_2 \mathrm{H}_4$ at the anode to form $\mathrm{N}_2(\mathrm{~g})$ and water, releasing 4 electrons to the anode.
B
At the cathode, $\mathrm{N}_2 \mathrm{H}_4$ breaks to $\mathrm{N}_2(\mathrm{~g})$ and nascent hydrogen released at the electrode reacts with oxygen to form water.
C
At the cathode, molecular oxygen gets converted to $\mathrm{OH}^{-}$.
D
Oxides of nitrogen are major by-products of the electrochemical process.
2
JEE Advanced 2021 Paper 2 Online
MCQ (More than One Correct Answer)
+4
-2
Change Language
Some standard electrode potentials at 298 K are given below :

Pb2+ /Pb = $$- $$0.13 V

Ni2+ /Ni = $$-$$ 0.24 V

Cd2+ /Cd = $$-$$ 0.40 V

Fe2+ /Fe = $$-$$ 0.44 V

To a solution containing 0.001 M of X2+ and 0.1 M of Y2+, the metal rods X and Y are inserted (at 298 K) and connected by a conducting wire. This resulted in dissolution of X. The correct combination(s) of X and Y, respectively, is(are)

(Given : Gas constant, R = 8.314 J K$$-$$ mol$$-$$1, Faraday constant, F = 96500 C mol$$-$$1)
A
Cd and Ni
B
Cd and Fe
C
Ni and Pb
D
Ni and Fe
3
JEE Advanced 2014 Paper 1 Offline
MCQ (More than One Correct Answer)
+3
-0
In a galvanic cell, the salt bridge
A
does not participate chemically in the cell reaction.
B
stops the diffusion of ions from one electrode to another.
C
is necessary for the occurrence of the cell reaction.
D
ensures mixing of the two electrolytic solutions.
4
IIT-JEE 2009 Paper 2 Offline
MCQ (More than One Correct Answer)
+4
-2

For the reduction of NO$$_3^ - $$ ion in an aqueous solution, E$$^0$$ is + 0.96 V. Values of E$$^0$$ for some metal ions are given below:

$$\matrix{ {{V^{2 + }}(aq.) + 2{e^ - } \to V} & {{E^0} = - 1.19\,V} \cr {F{e^{3 + }}(aq.) + 3{e^ - } \to Fe} & {{E^0} = - 0.04\,V} \cr {A{u^{3 + }}(aq) + 3{e^ - } \to Au} & {{E^0} = + 1.40\,V} \cr {H{g^{2 + }}(aq) + 2{e^ - } \to Hg} & {{E^0} = + 0.86\,V} \cr } $$

The pair(s) of metals that is (are) oxidized by NO$$_3^ - $$ in aqueous solution is(are)

A
V and Hg
B
Hg and Fe
C
Fe and Au
D
Fe and V
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