In electrolysis of NaCl when Pt electrode is taken then H2 is liberated at cathode while with Hg electrode it forms sodium amalgam
Hg is more inert than Pt
more voltage is required to reduce H+ at Hg than at Pt
Na is dissolved in Hg while it does not dissolve in Pt
concentration of H+ ions is larger when Pt electrode is taken
On the basis of the information available from the reaction,
G = -827 kJ mol-1 of O2, the minimum emf required to carry out an electrolysis of Al2O3 is (F = 96500 mol-1)
2.14 V
4.28 V
6.42 V
8.56 V
4.5 g of aluminium (atomic mass 27 u) is deposited at cathode from Al3+ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ions in solution by the same quantity of electric charge will be
44.8 L
11.2 L
22.4 L
5.6 L
D.
5.6 L
After passing same amount of electricity equal gram equivalent of substances deposited or dissolved.
So, gram equivalent of aluminium = gram equivalent of hydrogen
Volume of H2 at STP = 5.6 L
For the electrolysis of aqua CuSO4 solution using inert Pt electrodes, the reaction on anode
Cu2+ + 2e- → Cu
2H2O → O2 + 4H++ 4e-
2H+ + 2e- → H2
If we mix a pentavalent impurity in a crystal lattice of Ge, what type of semiconductor formation will occur?
p-type
n-type
Both (a) and (b)
None of these
If 'F' is Faraday and 'N' is Avogadro number, then charge of electron can be expressed as
F × N
F2N
By passing 9.65 A current for 16 min 40 s, the volume of O2 liberated at STP will be
280mL
560mL
1120mL
2240mL
By diluting a weak electrolyte, specific conductivity (Kc) and equivalent conductivity (Λc) change as
both increase
Kc increase λc decrease
Kc decrease λc increase
both decrease
In Daniel cell, anode and cathode are respectively
Zn| Zn2+ and Cu2+|Cu
Cu2+|Cu and Zn| Zn2+
Fe|Fe2+ and Cu2+|Cu
Cu2+|Cu and Fe|Fe2+
Copper sulphate solution is electrolysed using copper electrode. The reaction taking place at anode is
H+ + e- → H
SO (aq) → SO4 + 2e-
Cu2+ + 2e- → Cu
Cu (s) → Cu2+ (aq) + 2e-