Advertisements
Advertisements
प्रश्न
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?
पर्याय
\[\ce{Na+ (aq) + e- -> Na (s); E^{Θ}_{cell} = - 2.71V}\]
\[\ce{2H2O (l) -> O2(g) + 4H+ (aq) + 4e^- ; E^{Θ}_{cell} = 1.23V}\]
\[\ce{H^+ (aq) + e^- -> 1/2 H2 (g); E^{Θ}_{cell} = 0.00V}\]
\[\ce{Cl^- (aq) -> 1/2 Cl2 (g) + e^- ; E^{Θ}_{cell} = 1.36V}\]
Advertisements
उत्तर
\[\ce{Cl^- (aq) -> 1/2 Cl2 (g) + e^- ; E^{Θ}_{cell} = 1.36V}\]
Explanation:
During electrolysis of aqueous
\[\ce{NaCl -> Na^+ + Cl^-}\]
\[\ce{H2O -> H+ + OH-}\]
\[\ce{Na+ + e- -> Na (E^{Θ}_{cell} = - 2.71V)}\]
\[\ce{H^+ e- -> 1/2 H2 E^{Θ}_{cell} = 0.00V}\]
At cathode,
\[\ce{H2O + e- -> 1/2 H2 + OH-}\]
At anode, two reactions are possible.
\[\ce{Cl^{-} -> 1/2 Cl2 + e- ; E^{Θ}_{cell} = 1.36V}\]
\[\ce{2H2O -> O2 + 4H+ + 4e- ; E^{Θ}_{cell} = 1.23V}\]
APPEARS IN
संबंधित प्रश्न
On calculating the strength of current in amperes if a charge of 840C (coulomb) passes through an electrolyte in 7 minutes, it will be
- 1
- 2
- 3
- 4
96500 coulombs correspond to the charge on how many electrons?
Write any four applications of electrochemical series
If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?
Suggest a list of metals that are extracted electrolytically.
A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?
Draw neat labelled diagram of electrolytic refining of blister copper
What is the ratio of volumes of H2 and O2 liberated during electrolysis of acidified water?
(A) 1 : 2
(B) 2 : 1
(C) 1 : 8
(D) 8 : 1
Electrolytic cell uses electrical energy to bring about ____________.
What will happen during the electrolysis of aqueous solution of \[\ce{CuSO4}\] by using platinum electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will deposit at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will dissolve at anode.
What will happen during the electrolysis of aqueous solution of CuSO4 in the presence of Cu electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will dissolve at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will deposit at anode.
Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.
Given `1/a` = 0.5 CM–1, R = 50 ohm, N = 1.0 then equivalent conductance of electrolytic cell is
Assertion (A): During electrolysis of aqueous copper sulphate solution using copper electrodes hydrogen gas is released at the cathode.
Reason (R): The electrode potential of Cu2+/Cu is greater than that of H+/H2.
Select the most appropriate answer from the options given below:
How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten Al2O3?
(Given: Molar mass of Aluminium is 27 g mol−1.)
