During electrolysis of aqueous `CuBr_(2)` using `Pt` electrode,A. `Br_(2)` gas is evolved at the anodeB. `Cu(s)` is deposited at the cathodeC. `Br_(2)` gas is evolved at anode and `H_(2)` gas at cathodeD. `H_(2)` gas is evolved at anode.

During electrolysis of aqueous `CuBr_(2)` using `Pt` electrode,A. `Br_

1.	During electrolysis of aqueous `CuBr_(2)` using `Pt` electrode,A. `Br_(2)` gas is evolved at the anodeB. `Cu(s)` is deposited at the cathodeC. `Br_(2)` gas is evolved at anode and `H_(2)` gas at cathodeD. `H_(2)` gas is evolved at anode.
Answer» Correct Answer - A::B (A,B) at cathode: `Cu^(2+)+2e^(-)toCu(s)` `underline(2Br^(-)+toBr_(2)2e^(-))` `Cu^(2+)+2Br^(-)toBr_(2)+Cu(s)`.

Discussion

No Comment Found

Related InterviewSolutions

Consider the cell `H_(2)(Pt)`|{:(H_(3)O^(+)(aq)),(pH= 5.03):}||{:(Ag^(+),),("xM"):}|Ag`. The measured EMF of the cell is 1.0V. What is the value of x? `[E_(Ag^(+),Ag)^(@) = +0.8V][T = 25^(@)C]`A. `2xx10^(-2)M`B. `2xx10^(-3)M`C. `1.5xx10^(-3)M`D. `1.5xx10^(-2)M`
`Pt|underset((p_(1)))(H_(2))|underset((1M))(H^(+))||underset((1M))(H^(+))|underset((p_(2)))(H_(2))|Pt` (where `p_(1)` and `p_(2)` are pressure) cell reaction cell reaction will be spontaneous if:A. `p_(1)=p_(2)`B. `p_(1)gtp_(2)`C. `p_(2)gtp_(1)`D. `p_(1)=1atm`
What will be the emf for the given cell ? `Pt|H_(2)(g,P_(1))|H^(+)(aq)|H_(2)(g,P_(2))|Pt`A. `(RT)/(F)log_(e)(p_(1))/(p_(2))`B. `(RT)/(2F)log_(e)(p_(1))/(p_(2))`C. `(RT)/(F)log_(e)(p_(2))/(p_(1))`D. `(RT)/(2F)log_(e)^(p_(2))/(p_(1))`
A galvanic cell is compsed of two hydrogen electrodes, one of which is a standard one. In which of the following solutions should the other electrode be immersed to get maximum emf? `K_(a)(CH_(3)COOH) = 2 xx 10^(-5)` ,`K_(a)(H_(3)PO_(4)) = 10^(-3)`.A. 0.1 M HClB. 0.1 M `CH_(3)COOH`C. `0.1M` `H_(2)PO_(4)`D. `0.1 M H_(2)SO_(4)`
Equinormal solutions of two weak acids `HA(pK_(a)=3)` and `HB(pK_(a)=5)` are each placed in contact with standard hydrogen electrode at `25^(@)C(T=298K)` when a cell is constructed by interconnecting them through a salt bridge find the e.m.f. of the cell.
Cadmium amalgam is prepared by electrolysis of a solution of `CdCl_(2)` using a mercury cathode. Find how long a current of 5 ampere should be passed in order to prepare 12% Cd-Hg amalgam on a cathode of 2 g mercury. At mass of Cd=112.40.
The number of electrons delivered at the cathode during electrolysis by a current of `1` ampere in 60 seconds is (charger on electron `= 1.60 xx 10^(-19)C`)A. `3.74xx10^(20)`B. `6.0xx10^(23)`C. `7.48xx10^(21)`D. `6.0xx10^(20)`
Which of the following statement is true for the electrochemical Daniell cell ?A. electrons flows from copper electrode to zinc electrode.B. Current flows from zinc electrode to copper electrode.C. Cations moves towards copper electrodes.D. cations moves towards zinc electrode.
the standard reduction potenital of a silver chloride electrode is 0.2 V and that of a silver electrode is 0.79 V. The maximum amount of AgCl that can dissolve in `10^(6)`L of a 0.1 M `AgNO_(3)` solution is:A. 0.5 mmolB. 1.0 mmolC. 2.0 mmolD. 2.5 mmol
A cell `Cu|Cu^(++)||Ag^(+)|Ag` initially contains `2MAg^(+)` and `2MCu^(++)` ions in 1 L electrolyte. The change in cell potential after the passage of 10 amp. Curret for 4825 sec is:A. `-0.00738V`B. `-1.00738V`C. `-0.0038V`D. none

During electrolysis of aqueous `CuBr_(2)` using `Pt` electrode,A. `Br_(2)` gas is evolved at the anodeB. `Cu(s)` is deposited at the cathodeC. `Br_(2)` gas is evolved at anode and `H_(2)` gas at cathodeD. `H_(2)` gas is evolved at anode.

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment