19905
One Faraday of electricity when passed through a solution of copper sulphate deposits
1 \(1\) mole of \(Cu\)
2 \(1\,\,gm\) atom of \(Cu\)
3 \(1\) molecule of \(Cu\)
4 \(1\,\,gm\) equivalent of \(Cu\)
Explanation:
(d)One Faraday\( = 1\,\,gm\) of equivalent of \(Cu\).
ELECTROCHEMISTRY
19906
When \(1\,coulomb\) of charge is passed through electrolyte solution, then the mass deposited is equal to
1 Equivalent weight
2 Atomic weight
3 Electrochemical equivalent
4 Chemical equivalent
Explanation:
(c)\(W = Zit\,\,;\,\,\,Z = \frac{E}{{96500}}\).
ELECTROCHEMISTRY
19907
The platinum electrodes were immersed in a solution of cupric sulphate and electric current passed through the solution. After some time it was found that colour of copper sulphate disappeared with evolution of gas at the electrode. The colourless solution contains
1 Platinum sulphate
2 Copper hydroxide
3 Copper sulphate
4 Sulphuric acid
Explanation:
(d)During electrolysis of \(CuS{O_4}\).\(C{u^{2 + }}\) gets discharged at cathode and \(O{H^ - }\)at anode. Thus solution becomes acidic due to excess of \({H^ + }\) and \(SO_4^{2 - }\) or \({H_2}S{O_4}\).
ELECTROCHEMISTRY
19908
On passing \(C\) ampere of electricity through a electrolyte solution for \(t\) second, \(m\) gram metal deposits on cathode. The equivalent weight \(E\) of the metal is
19905
One Faraday of electricity when passed through a solution of copper sulphate deposits
1 \(1\) mole of \(Cu\)
2 \(1\,\,gm\) atom of \(Cu\)
3 \(1\) molecule of \(Cu\)
4 \(1\,\,gm\) equivalent of \(Cu\)
Explanation:
(d)One Faraday\( = 1\,\,gm\) of equivalent of \(Cu\).
ELECTROCHEMISTRY
19906
When \(1\,coulomb\) of charge is passed through electrolyte solution, then the mass deposited is equal to
1 Equivalent weight
2 Atomic weight
3 Electrochemical equivalent
4 Chemical equivalent
Explanation:
(c)\(W = Zit\,\,;\,\,\,Z = \frac{E}{{96500}}\).
ELECTROCHEMISTRY
19907
The platinum electrodes were immersed in a solution of cupric sulphate and electric current passed through the solution. After some time it was found that colour of copper sulphate disappeared with evolution of gas at the electrode. The colourless solution contains
1 Platinum sulphate
2 Copper hydroxide
3 Copper sulphate
4 Sulphuric acid
Explanation:
(d)During electrolysis of \(CuS{O_4}\).\(C{u^{2 + }}\) gets discharged at cathode and \(O{H^ - }\)at anode. Thus solution becomes acidic due to excess of \({H^ + }\) and \(SO_4^{2 - }\) or \({H_2}S{O_4}\).
ELECTROCHEMISTRY
19908
On passing \(C\) ampere of electricity through a electrolyte solution for \(t\) second, \(m\) gram metal deposits on cathode. The equivalent weight \(E\) of the metal is
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
ELECTROCHEMISTRY
19905
One Faraday of electricity when passed through a solution of copper sulphate deposits
1 \(1\) mole of \(Cu\)
2 \(1\,\,gm\) atom of \(Cu\)
3 \(1\) molecule of \(Cu\)
4 \(1\,\,gm\) equivalent of \(Cu\)
Explanation:
(d)One Faraday\( = 1\,\,gm\) of equivalent of \(Cu\).
ELECTROCHEMISTRY
19906
When \(1\,coulomb\) of charge is passed through electrolyte solution, then the mass deposited is equal to
1 Equivalent weight
2 Atomic weight
3 Electrochemical equivalent
4 Chemical equivalent
Explanation:
(c)\(W = Zit\,\,;\,\,\,Z = \frac{E}{{96500}}\).
ELECTROCHEMISTRY
19907
The platinum electrodes were immersed in a solution of cupric sulphate and electric current passed through the solution. After some time it was found that colour of copper sulphate disappeared with evolution of gas at the electrode. The colourless solution contains
1 Platinum sulphate
2 Copper hydroxide
3 Copper sulphate
4 Sulphuric acid
Explanation:
(d)During electrolysis of \(CuS{O_4}\).\(C{u^{2 + }}\) gets discharged at cathode and \(O{H^ - }\)at anode. Thus solution becomes acidic due to excess of \({H^ + }\) and \(SO_4^{2 - }\) or \({H_2}S{O_4}\).
ELECTROCHEMISTRY
19908
On passing \(C\) ampere of electricity through a electrolyte solution for \(t\) second, \(m\) gram metal deposits on cathode. The equivalent weight \(E\) of the metal is
19905
One Faraday of electricity when passed through a solution of copper sulphate deposits
1 \(1\) mole of \(Cu\)
2 \(1\,\,gm\) atom of \(Cu\)
3 \(1\) molecule of \(Cu\)
4 \(1\,\,gm\) equivalent of \(Cu\)
Explanation:
(d)One Faraday\( = 1\,\,gm\) of equivalent of \(Cu\).
ELECTROCHEMISTRY
19906
When \(1\,coulomb\) of charge is passed through electrolyte solution, then the mass deposited is equal to
1 Equivalent weight
2 Atomic weight
3 Electrochemical equivalent
4 Chemical equivalent
Explanation:
(c)\(W = Zit\,\,;\,\,\,Z = \frac{E}{{96500}}\).
ELECTROCHEMISTRY
19907
The platinum electrodes were immersed in a solution of cupric sulphate and electric current passed through the solution. After some time it was found that colour of copper sulphate disappeared with evolution of gas at the electrode. The colourless solution contains
1 Platinum sulphate
2 Copper hydroxide
3 Copper sulphate
4 Sulphuric acid
Explanation:
(d)During electrolysis of \(CuS{O_4}\).\(C{u^{2 + }}\) gets discharged at cathode and \(O{H^ - }\)at anode. Thus solution becomes acidic due to excess of \({H^ + }\) and \(SO_4^{2 - }\) or \({H_2}S{O_4}\).
ELECTROCHEMISTRY
19908
On passing \(C\) ampere of electricity through a electrolyte solution for \(t\) second, \(m\) gram metal deposits on cathode. The equivalent weight \(E\) of the metal is