01. Faraday's Law
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ELECTROCHEMISTRY

276012 Which of the following conversions involves gain of 5 electrons per ion?

1 $\mathrm{MnO}_{4}^{-} \rightarrow \mathrm{Mn}^{2+}$
2 $\mathrm{CrO}_{4}^{2-} \rightarrow \mathrm{Cr}^{3+}$
3 $\mathrm{MnO}_{4}^{2-} \rightarrow \mathrm{MnO}_{2}$
4 $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \rightarrow 2 \mathrm{Cr}^{3+}$
SRMJEEE-2013
ELECTROCHEMISTRY

276014 A $200 \mathrm{~W}, 100 \mathrm{~V}$ bulb is connected in series with an electrolytic cell. If an aqueous solution of an Sn-salt is electrolysed for $5 \mathrm{hrs}, 11.1 \mathrm{~g}$ of $\mathrm{Sn}$ gets deposited. The chemical formula of the compound is ......... (Given atomic weight of Sn is $118.7 \mathrm{~g} \mathrm{~mol}^{-1}$ )

1 $\mathrm{SnO}$
2 $\mathrm{SnC}_{2}$
3 $\mathrm{SnC}_{4}$
4 $\mathrm{SnO}_{2}$
Shift-I
ELECTROCHEMISTRY

276015 How much current is required to produce $\mathrm{H}_{2}$ gas at the rate of $1 \mathrm{cc} / \mathrm{sec}$ under STP?

1 $33 \mathrm{~A}$
2 $6.0 \mathrm{~A}$
3 $7.9 \mathrm{~A}$
4 $8.61 \mathrm{~A}$
Shift-II
ELECTROCHEMISTRY

276016 When a current of $10 \mathrm{~A}$ is passes through molten $\mathrm{AlCl}_{3}$ for 1.608 minutes. The mass of $\mathrm{Al}$ deposited will be- [Atomic mass of $\mathrm{Al}=\mathbf{2 7} \mathrm{g}$ ]

1 $0.09 \mathrm{~g}$
2 $0.81 \mathrm{~g}$
3 $1.35 \mathrm{~g}$
4 $0.27 \mathrm{~g}$
AP-EAPCET 19-08-2021 Shift-I
ELECTROCHEMISTRY

276017 An electric current is passed through silver and water voltmeters connected in series. The cathode of silver voltmeter weighed $0.054 \mathrm{~g}$ more after the electrolysis. The volume of $\mathrm{O}_{2}$ liberated is

1 $5.6 \mathrm{~cm}^{3}$
2 $11.2 \mathrm{~cm}^{3}$
3 $22.4 \mathrm{~cm}^{3}$
4 $2.8 \mathrm{~cm}^{3}$
COMEDK-2012
NEET DIGITAL LIBRARY
ELECTROCHEMISTRY

276012 Which of the following conversions involves gain of 5 electrons per ion?

1 $\mathrm{MnO}_{4}^{-} \rightarrow \mathrm{Mn}^{2+}$
2 $\mathrm{CrO}_{4}^{2-} \rightarrow \mathrm{Cr}^{3+}$
3 $\mathrm{MnO}_{4}^{2-} \rightarrow \mathrm{MnO}_{2}$
4 $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \rightarrow 2 \mathrm{Cr}^{3+}$
SRMJEEE-2013
ELECTROCHEMISTRY

276014 A $200 \mathrm{~W}, 100 \mathrm{~V}$ bulb is connected in series with an electrolytic cell. If an aqueous solution of an Sn-salt is electrolysed for $5 \mathrm{hrs}, 11.1 \mathrm{~g}$ of $\mathrm{Sn}$ gets deposited. The chemical formula of the compound is ......... (Given atomic weight of Sn is $118.7 \mathrm{~g} \mathrm{~mol}^{-1}$ )

1 $\mathrm{SnO}$
2 $\mathrm{SnC}_{2}$
3 $\mathrm{SnC}_{4}$
4 $\mathrm{SnO}_{2}$
Shift-I
ELECTROCHEMISTRY

276015 How much current is required to produce $\mathrm{H}_{2}$ gas at the rate of $1 \mathrm{cc} / \mathrm{sec}$ under STP?

1 $33 \mathrm{~A}$
2 $6.0 \mathrm{~A}$
3 $7.9 \mathrm{~A}$
4 $8.61 \mathrm{~A}$
Shift-II
ELECTROCHEMISTRY

276016 When a current of $10 \mathrm{~A}$ is passes through molten $\mathrm{AlCl}_{3}$ for 1.608 minutes. The mass of $\mathrm{Al}$ deposited will be- [Atomic mass of $\mathrm{Al}=\mathbf{2 7} \mathrm{g}$ ]

1 $0.09 \mathrm{~g}$
2 $0.81 \mathrm{~g}$
3 $1.35 \mathrm{~g}$
4 $0.27 \mathrm{~g}$
AP-EAPCET 19-08-2021 Shift-I
ELECTROCHEMISTRY

276017 An electric current is passed through silver and water voltmeters connected in series. The cathode of silver voltmeter weighed $0.054 \mathrm{~g}$ more after the electrolysis. The volume of $\mathrm{O}_{2}$ liberated is

1 $5.6 \mathrm{~cm}^{3}$
2 $11.2 \mathrm{~cm}^{3}$
3 $22.4 \mathrm{~cm}^{3}$
4 $2.8 \mathrm{~cm}^{3}$
COMEDK-2012
Join With Us for More Updates
ELECTROCHEMISTRY

276012 Which of the following conversions involves gain of 5 electrons per ion?

1 $\mathrm{MnO}_{4}^{-} \rightarrow \mathrm{Mn}^{2+}$
2 $\mathrm{CrO}_{4}^{2-} \rightarrow \mathrm{Cr}^{3+}$
3 $\mathrm{MnO}_{4}^{2-} \rightarrow \mathrm{MnO}_{2}$
4 $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \rightarrow 2 \mathrm{Cr}^{3+}$
SRMJEEE-2013
ELECTROCHEMISTRY

276014 A $200 \mathrm{~W}, 100 \mathrm{~V}$ bulb is connected in series with an electrolytic cell. If an aqueous solution of an Sn-salt is electrolysed for $5 \mathrm{hrs}, 11.1 \mathrm{~g}$ of $\mathrm{Sn}$ gets deposited. The chemical formula of the compound is ......... (Given atomic weight of Sn is $118.7 \mathrm{~g} \mathrm{~mol}^{-1}$ )

1 $\mathrm{SnO}$
2 $\mathrm{SnC}_{2}$
3 $\mathrm{SnC}_{4}$
4 $\mathrm{SnO}_{2}$
Shift-I
ELECTROCHEMISTRY

276015 How much current is required to produce $\mathrm{H}_{2}$ gas at the rate of $1 \mathrm{cc} / \mathrm{sec}$ under STP?

1 $33 \mathrm{~A}$
2 $6.0 \mathrm{~A}$
3 $7.9 \mathrm{~A}$
4 $8.61 \mathrm{~A}$
Shift-II
ELECTROCHEMISTRY

276016 When a current of $10 \mathrm{~A}$ is passes through molten $\mathrm{AlCl}_{3}$ for 1.608 minutes. The mass of $\mathrm{Al}$ deposited will be- [Atomic mass of $\mathrm{Al}=\mathbf{2 7} \mathrm{g}$ ]

1 $0.09 \mathrm{~g}$
2 $0.81 \mathrm{~g}$
3 $1.35 \mathrm{~g}$
4 $0.27 \mathrm{~g}$
AP-EAPCET 19-08-2021 Shift-I
ELECTROCHEMISTRY

276017 An electric current is passed through silver and water voltmeters connected in series. The cathode of silver voltmeter weighed $0.054 \mathrm{~g}$ more after the electrolysis. The volume of $\mathrm{O}_{2}$ liberated is

1 $5.6 \mathrm{~cm}^{3}$
2 $11.2 \mathrm{~cm}^{3}$
3 $22.4 \mathrm{~cm}^{3}$
4 $2.8 \mathrm{~cm}^{3}$
COMEDK-2012
For More Updates join with Us
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ELECTROCHEMISTRY

276012 Which of the following conversions involves gain of 5 electrons per ion?

1 $\mathrm{MnO}_{4}^{-} \rightarrow \mathrm{Mn}^{2+}$
2 $\mathrm{CrO}_{4}^{2-} \rightarrow \mathrm{Cr}^{3+}$
3 $\mathrm{MnO}_{4}^{2-} \rightarrow \mathrm{MnO}_{2}$
4 $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \rightarrow 2 \mathrm{Cr}^{3+}$
SRMJEEE-2013
ELECTROCHEMISTRY

276014 A $200 \mathrm{~W}, 100 \mathrm{~V}$ bulb is connected in series with an electrolytic cell. If an aqueous solution of an Sn-salt is electrolysed for $5 \mathrm{hrs}, 11.1 \mathrm{~g}$ of $\mathrm{Sn}$ gets deposited. The chemical formula of the compound is ......... (Given atomic weight of Sn is $118.7 \mathrm{~g} \mathrm{~mol}^{-1}$ )

1 $\mathrm{SnO}$
2 $\mathrm{SnC}_{2}$
3 $\mathrm{SnC}_{4}$
4 $\mathrm{SnO}_{2}$
Shift-I
ELECTROCHEMISTRY

276015 How much current is required to produce $\mathrm{H}_{2}$ gas at the rate of $1 \mathrm{cc} / \mathrm{sec}$ under STP?

1 $33 \mathrm{~A}$
2 $6.0 \mathrm{~A}$
3 $7.9 \mathrm{~A}$
4 $8.61 \mathrm{~A}$
Shift-II
ELECTROCHEMISTRY

276016 When a current of $10 \mathrm{~A}$ is passes through molten $\mathrm{AlCl}_{3}$ for 1.608 minutes. The mass of $\mathrm{Al}$ deposited will be- [Atomic mass of $\mathrm{Al}=\mathbf{2 7} \mathrm{g}$ ]

1 $0.09 \mathrm{~g}$
2 $0.81 \mathrm{~g}$
3 $1.35 \mathrm{~g}$
4 $0.27 \mathrm{~g}$
AP-EAPCET 19-08-2021 Shift-I
ELECTROCHEMISTRY

276017 An electric current is passed through silver and water voltmeters connected in series. The cathode of silver voltmeter weighed $0.054 \mathrm{~g}$ more after the electrolysis. The volume of $\mathrm{O}_{2}$ liberated is

1 $5.6 \mathrm{~cm}^{3}$
2 $11.2 \mathrm{~cm}^{3}$
3 $22.4 \mathrm{~cm}^{3}$
4 $2.8 \mathrm{~cm}^{3}$
COMEDK-2012
NEET DIGITAL LIBRARY
ELECTROCHEMISTRY

276012 Which of the following conversions involves gain of 5 electrons per ion?

1 $\mathrm{MnO}_{4}^{-} \rightarrow \mathrm{Mn}^{2+}$
2 $\mathrm{CrO}_{4}^{2-} \rightarrow \mathrm{Cr}^{3+}$
3 $\mathrm{MnO}_{4}^{2-} \rightarrow \mathrm{MnO}_{2}$
4 $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \rightarrow 2 \mathrm{Cr}^{3+}$
SRMJEEE-2013
ELECTROCHEMISTRY

276014 A $200 \mathrm{~W}, 100 \mathrm{~V}$ bulb is connected in series with an electrolytic cell. If an aqueous solution of an Sn-salt is electrolysed for $5 \mathrm{hrs}, 11.1 \mathrm{~g}$ of $\mathrm{Sn}$ gets deposited. The chemical formula of the compound is ......... (Given atomic weight of Sn is $118.7 \mathrm{~g} \mathrm{~mol}^{-1}$ )

1 $\mathrm{SnO}$
2 $\mathrm{SnC}_{2}$
3 $\mathrm{SnC}_{4}$
4 $\mathrm{SnO}_{2}$
Shift-I
ELECTROCHEMISTRY

276015 How much current is required to produce $\mathrm{H}_{2}$ gas at the rate of $1 \mathrm{cc} / \mathrm{sec}$ under STP?

1 $33 \mathrm{~A}$
2 $6.0 \mathrm{~A}$
3 $7.9 \mathrm{~A}$
4 $8.61 \mathrm{~A}$
Shift-II
ELECTROCHEMISTRY

276016 When a current of $10 \mathrm{~A}$ is passes through molten $\mathrm{AlCl}_{3}$ for 1.608 minutes. The mass of $\mathrm{Al}$ deposited will be- [Atomic mass of $\mathrm{Al}=\mathbf{2 7} \mathrm{g}$ ]

1 $0.09 \mathrm{~g}$
2 $0.81 \mathrm{~g}$
3 $1.35 \mathrm{~g}$
4 $0.27 \mathrm{~g}$
AP-EAPCET 19-08-2021 Shift-I
ELECTROCHEMISTRY

276017 An electric current is passed through silver and water voltmeters connected in series. The cathode of silver voltmeter weighed $0.054 \mathrm{~g}$ more after the electrolysis. The volume of $\mathrm{O}_{2}$ liberated is

1 $5.6 \mathrm{~cm}^{3}$
2 $11.2 \mathrm{~cm}^{3}$
3 $22.4 \mathrm{~cm}^{3}$
4 $2.8 \mathrm{~cm}^{3}$
COMEDK-2012