19934
When \(96500 \) coulomb of electricity is passed through a copper sulphate solution, the amount of copper deposited will be ............... \(\mathrm{mol}\)
1 \(0.25\)
2 \(0.50\)
3 \(1\)
4 \(2\)
Explanation:
(b) \(31.75\,g\) copper gets deposited at cathode on passing \(96500\) coulomb charge. We know that \( 31.75\,gm \) of \(Cu \) is equal to \( 0.5\,mole\) of \(Cu\) deposited at cathode on passing \( 1\,F \) of current.
ELECTROCHEMISTRY
19935
During electrolysis of fused aluminium chloride \(0.9\,gm\) of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be .............. \(\mathrm{litres}\)
1 \(2.24\)
2 \(11.2\)
3 \(1.12\)
4 \(5.6\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19936
Faraday has the dimensions of
1 Coulombs
2 Coulomb equivalent
3 Coulomb per equivalent
4 Coulomb per degree Kelvin
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19937
The required charge for one equivalent weight of silver deposite on cathode is
1 \(9.65 \times {10^7}\,C\)
2 \(9.65 \times {10^4}\,C\)
3 \(9.65 \times {10^3}\,C\)
4 \(9.65 \times {10^5}\,C\)
Explanation:
(b)For deposition of one equivalent silver required charged is \(96500\,C.\)
19934
When \(96500 \) coulomb of electricity is passed through a copper sulphate solution, the amount of copper deposited will be ............... \(\mathrm{mol}\)
1 \(0.25\)
2 \(0.50\)
3 \(1\)
4 \(2\)
Explanation:
(b) \(31.75\,g\) copper gets deposited at cathode on passing \(96500\) coulomb charge. We know that \( 31.75\,gm \) of \(Cu \) is equal to \( 0.5\,mole\) of \(Cu\) deposited at cathode on passing \( 1\,F \) of current.
ELECTROCHEMISTRY
19935
During electrolysis of fused aluminium chloride \(0.9\,gm\) of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be .............. \(\mathrm{litres}\)
1 \(2.24\)
2 \(11.2\)
3 \(1.12\)
4 \(5.6\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19936
Faraday has the dimensions of
1 Coulombs
2 Coulomb equivalent
3 Coulomb per equivalent
4 Coulomb per degree Kelvin
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19937
The required charge for one equivalent weight of silver deposite on cathode is
1 \(9.65 \times {10^7}\,C\)
2 \(9.65 \times {10^4}\,C\)
3 \(9.65 \times {10^3}\,C\)
4 \(9.65 \times {10^5}\,C\)
Explanation:
(b)For deposition of one equivalent silver required charged is \(96500\,C.\)
19934
When \(96500 \) coulomb of electricity is passed through a copper sulphate solution, the amount of copper deposited will be ............... \(\mathrm{mol}\)
1 \(0.25\)
2 \(0.50\)
3 \(1\)
4 \(2\)
Explanation:
(b) \(31.75\,g\) copper gets deposited at cathode on passing \(96500\) coulomb charge. We know that \( 31.75\,gm \) of \(Cu \) is equal to \( 0.5\,mole\) of \(Cu\) deposited at cathode on passing \( 1\,F \) of current.
ELECTROCHEMISTRY
19935
During electrolysis of fused aluminium chloride \(0.9\,gm\) of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be .............. \(\mathrm{litres}\)
1 \(2.24\)
2 \(11.2\)
3 \(1.12\)
4 \(5.6\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19936
Faraday has the dimensions of
1 Coulombs
2 Coulomb equivalent
3 Coulomb per equivalent
4 Coulomb per degree Kelvin
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19937
The required charge for one equivalent weight of silver deposite on cathode is
1 \(9.65 \times {10^7}\,C\)
2 \(9.65 \times {10^4}\,C\)
3 \(9.65 \times {10^3}\,C\)
4 \(9.65 \times {10^5}\,C\)
Explanation:
(b)For deposition of one equivalent silver required charged is \(96500\,C.\)
19934
When \(96500 \) coulomb of electricity is passed through a copper sulphate solution, the amount of copper deposited will be ............... \(\mathrm{mol}\)
1 \(0.25\)
2 \(0.50\)
3 \(1\)
4 \(2\)
Explanation:
(b) \(31.75\,g\) copper gets deposited at cathode on passing \(96500\) coulomb charge. We know that \( 31.75\,gm \) of \(Cu \) is equal to \( 0.5\,mole\) of \(Cu\) deposited at cathode on passing \( 1\,F \) of current.
ELECTROCHEMISTRY
19935
During electrolysis of fused aluminium chloride \(0.9\,gm\) of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be .............. \(\mathrm{litres}\)
1 \(2.24\)
2 \(11.2\)
3 \(1.12\)
4 \(5.6\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19936
Faraday has the dimensions of
1 Coulombs
2 Coulomb equivalent
3 Coulomb per equivalent
4 Coulomb per degree Kelvin
Explanation:
It’s obvious.
ELECTROCHEMISTRY
19937
The required charge for one equivalent weight of silver deposite on cathode is
1 \(9.65 \times {10^7}\,C\)
2 \(9.65 \times {10^4}\,C\)
3 \(9.65 \times {10^3}\,C\)
4 \(9.65 \times {10^5}\,C\)
Explanation:
(b)For deposition of one equivalent silver required charged is \(96500\,C.\)
