The passage of current through a solution of certain electrolye results in the evolution of H2 at cathode and Cl2 at anode. The electrolytic solution is -
In an electrolytic cell current flows from -
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When an aqueous solution of H2SO4 is electrolysed, the ion discharged at anode is-
1 mole of Al is deposited by X coulomb of electricity passing through aluminium nitrate solution. The number of moles of silver deposited by X coulomb of electricity from silver nitrate solution is-
A solution of Na2SO4 in water is electrolysed using Pt electrodes.The products at the cathode and anode are respectively -
In electrolysis of a fused salt, the weight deposited on an electrode will not depend on-
The electrolysis of a solution resulted in the formation of H2 at the cathode and Cl2 at the anode. The liquid is-
Which loses charge at cathode-
In the electrolysis of CuSO4, the reaction :
Cu2+ + 2e¯ → Cu, takes place at :
If mercury is used as cathode in the electrolysis of aqueous NaCl solution, the ions discharged at cathode are-
The specific conductance of a solution is 0.3568 ohm-1. When placed in a cell the conductance is 0.0268 ohm-1. The cell constant is-
A conductance cell was filled with a 0.02 M KCl solution which has a specific conductance of 2.768 × 10-3 ohm-1 cm-1. If its resistance is 82.4 ohm at 25ºC, the cell constant is-
The variation of equivalent conductance vs decrease in concentration of a strong electrolyte is correctly given in the plot -
Which of the following solutions has the highest equivalent conductance ?
The resistance of 0.01N solution of an electrolyte AB at 328K is 100 ohm. The specific conductance of solution is (cell constant = 1cm-1) -
For an electrolytic solution of 0.05 mol L-1, the conductivity has been found to be 0.0110 Scm-1.The molar conductivity is-
Two electrodes are fitted in conductance cell 1.5 cm apart while the area of cross section of each electrode is 0.75 cm2. The cell constant is-
The best conductor of electricity is in 1M solution of-
A certain current liberates 0.504 g of H2 in 2 hours. How many grams of copper can be liberated by the same current flowing for the same time in CuSO4 solution -
A currnet of 2.6 ampere is passed through CuSO4 solution for 6 minutes 20 seconds. The amount of Cu deposited is (At. wt. of Cu = 63.5, Faraday = 96500 C)-
Three Faradays of electricity are passed through molten Al2O3, aqueous solution of CuSO4 and molten NaCl taken in three different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of-
The quantity of electricity required to liberate 0.01g equivalent of an element at the electrode is-
The unit of electrochemical equivalent is-
One faraday of electricity will liberate one mole of metal from a solution of-
The number of faraday required to generate 1 mole of Mg from MgCl2 is-
One gm metal M+2 was discharged by the passage of 1.81×1022 electrons. What is the atomic weight of metal?
One mole of electron passes through each of the solution of AgNO3, CuSO4 and AlCl3 when Ag, Cu and Al are deposited at cathode. The molar ratio of Ag, Cu and Al deposited are
Salts of A (atomic weight = 7), B (atomic weight = 27) and C (atomic weight = 48) were electrolysed under identical conditions using the same quantity of electricity. It was found that when 2.1 g of A was deposited, the weights of B and C deposited were 2.7 and 7.2 g. The valencies of A, B and C respectively are
The density of Cu is 8.94 g cm–3. The quantity of electricity needed to plate an area 10 cm × 10cm to a thickness of 10-2 cm using CuSO4 solution would be
During electrolysis of an aqueous solution of sodium sulphate if 2.4 L of oxygen at STP was liberated at anode. The volume of hydrogen at STP, liberated at cathode would be :
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