19808
If in a voltaic cell \(5\,gm\) of zinc is consumed, then we get how many ampere hours ?(Given that \(E.C.E.\) of \(Zn\) is \(3.387 \times {10^{ - 7}}\,kg/coulomb\))
19809
The current flowing in a copper voltameter is \(1.6\, A\). The number of \(C{u^{ + + }}\) ions deposited at the cathode per minute are
1 \(1.5 \times {10^{20}}\)
2 \(3 \times {10^{20}}\)
3 \(6 \times {10^{20}}\)
4 \(1 \times {10^{19}}\)
Explanation:
(b) Charge \(Q = I t\) = \(1.6 × 60\) = \(96\, C\) Let \(n\) be the number of \(C{u^{ + 2}}\) ions, then \(ne = Q \Rightarrow n = \frac{Q}{e} = \frac{{96}}{{2 \times 1.6 \times {{10}^{ - 19}}}} = 3 \times {10^{20}}\)
ELECTROCHEMISTRY
19810
In a copper voltameter experiment, current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. Amount of copper deposited will be
1 Same
2 One-fourth the previous value
3 Four times the previous value
4 \(\frac{1}{{16}}th\) of the previous value
Explanation:
(a) In the first case, \(Zi\,t = m\) In the second case, \(Z \times \frac{i}{4} \times 4t = m\)
ELECTROCHEMISTRY
19811
The Avogadro's number is \(6 \times {10^{23}}\) per gm mole and electronic charge is \(1.6 \times {10^{ - 19}}C\). The Faraday's number is
19808
If in a voltaic cell \(5\,gm\) of zinc is consumed, then we get how many ampere hours ?(Given that \(E.C.E.\) of \(Zn\) is \(3.387 \times {10^{ - 7}}\,kg/coulomb\))
19809
The current flowing in a copper voltameter is \(1.6\, A\). The number of \(C{u^{ + + }}\) ions deposited at the cathode per minute are
1 \(1.5 \times {10^{20}}\)
2 \(3 \times {10^{20}}\)
3 \(6 \times {10^{20}}\)
4 \(1 \times {10^{19}}\)
Explanation:
(b) Charge \(Q = I t\) = \(1.6 × 60\) = \(96\, C\) Let \(n\) be the number of \(C{u^{ + 2}}\) ions, then \(ne = Q \Rightarrow n = \frac{Q}{e} = \frac{{96}}{{2 \times 1.6 \times {{10}^{ - 19}}}} = 3 \times {10^{20}}\)
ELECTROCHEMISTRY
19810
In a copper voltameter experiment, current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. Amount of copper deposited will be
1 Same
2 One-fourth the previous value
3 Four times the previous value
4 \(\frac{1}{{16}}th\) of the previous value
Explanation:
(a) In the first case, \(Zi\,t = m\) In the second case, \(Z \times \frac{i}{4} \times 4t = m\)
ELECTROCHEMISTRY
19811
The Avogadro's number is \(6 \times {10^{23}}\) per gm mole and electronic charge is \(1.6 \times {10^{ - 19}}C\). The Faraday's number is
NEET Test Series from KOTA - 10 Papers In MS WORD
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ELECTROCHEMISTRY
19808
If in a voltaic cell \(5\,gm\) of zinc is consumed, then we get how many ampere hours ?(Given that \(E.C.E.\) of \(Zn\) is \(3.387 \times {10^{ - 7}}\,kg/coulomb\))
19809
The current flowing in a copper voltameter is \(1.6\, A\). The number of \(C{u^{ + + }}\) ions deposited at the cathode per minute are
1 \(1.5 \times {10^{20}}\)
2 \(3 \times {10^{20}}\)
3 \(6 \times {10^{20}}\)
4 \(1 \times {10^{19}}\)
Explanation:
(b) Charge \(Q = I t\) = \(1.6 × 60\) = \(96\, C\) Let \(n\) be the number of \(C{u^{ + 2}}\) ions, then \(ne = Q \Rightarrow n = \frac{Q}{e} = \frac{{96}}{{2 \times 1.6 \times {{10}^{ - 19}}}} = 3 \times {10^{20}}\)
ELECTROCHEMISTRY
19810
In a copper voltameter experiment, current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. Amount of copper deposited will be
1 Same
2 One-fourth the previous value
3 Four times the previous value
4 \(\frac{1}{{16}}th\) of the previous value
Explanation:
(a) In the first case, \(Zi\,t = m\) In the second case, \(Z \times \frac{i}{4} \times 4t = m\)
ELECTROCHEMISTRY
19811
The Avogadro's number is \(6 \times {10^{23}}\) per gm mole and electronic charge is \(1.6 \times {10^{ - 19}}C\). The Faraday's number is
19808
If in a voltaic cell \(5\,gm\) of zinc is consumed, then we get how many ampere hours ?(Given that \(E.C.E.\) of \(Zn\) is \(3.387 \times {10^{ - 7}}\,kg/coulomb\))
19809
The current flowing in a copper voltameter is \(1.6\, A\). The number of \(C{u^{ + + }}\) ions deposited at the cathode per minute are
1 \(1.5 \times {10^{20}}\)
2 \(3 \times {10^{20}}\)
3 \(6 \times {10^{20}}\)
4 \(1 \times {10^{19}}\)
Explanation:
(b) Charge \(Q = I t\) = \(1.6 × 60\) = \(96\, C\) Let \(n\) be the number of \(C{u^{ + 2}}\) ions, then \(ne = Q \Rightarrow n = \frac{Q}{e} = \frac{{96}}{{2 \times 1.6 \times {{10}^{ - 19}}}} = 3 \times {10^{20}}\)
ELECTROCHEMISTRY
19810
In a copper voltameter experiment, current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. Amount of copper deposited will be
1 Same
2 One-fourth the previous value
3 Four times the previous value
4 \(\frac{1}{{16}}th\) of the previous value
Explanation:
(a) In the first case, \(Zi\,t = m\) In the second case, \(Z \times \frac{i}{4} \times 4t = m\)
ELECTROCHEMISTRY
19811
The Avogadro's number is \(6 \times {10^{23}}\) per gm mole and electronic charge is \(1.6 \times {10^{ - 19}}C\). The Faraday's number is
19808
If in a voltaic cell \(5\,gm\) of zinc is consumed, then we get how many ampere hours ?(Given that \(E.C.E.\) of \(Zn\) is \(3.387 \times {10^{ - 7}}\,kg/coulomb\))
19809
The current flowing in a copper voltameter is \(1.6\, A\). The number of \(C{u^{ + + }}\) ions deposited at the cathode per minute are
1 \(1.5 \times {10^{20}}\)
2 \(3 \times {10^{20}}\)
3 \(6 \times {10^{20}}\)
4 \(1 \times {10^{19}}\)
Explanation:
(b) Charge \(Q = I t\) = \(1.6 × 60\) = \(96\, C\) Let \(n\) be the number of \(C{u^{ + 2}}\) ions, then \(ne = Q \Rightarrow n = \frac{Q}{e} = \frac{{96}}{{2 \times 1.6 \times {{10}^{ - 19}}}} = 3 \times {10^{20}}\)
ELECTROCHEMISTRY
19810
In a copper voltameter experiment, current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. Amount of copper deposited will be
1 Same
2 One-fourth the previous value
3 Four times the previous value
4 \(\frac{1}{{16}}th\) of the previous value
Explanation:
(a) In the first case, \(Zi\,t = m\) In the second case, \(Z \times \frac{i}{4} \times 4t = m\)
ELECTROCHEMISTRY
19811
The Avogadro's number is \(6 \times {10^{23}}\) per gm mole and electronic charge is \(1.6 \times {10^{ - 19}}C\). The Faraday's number is