Home
Class 11
CHEMISTRY
A 1 M solution of H2SO4 is electrolysed....

A 1 M solution of `H_2SO_4` is electrolysed. Select correct statement in respect of products obtain at anode and cathode respectively:
Given : `2SO_4^(2-) toS_2O_8^(2-)+2e^-,E^(@)=-2.01V`
`H_2O(l)to2H^+(aq)+1//2O_2(g)+2e^-,E^(@)=-1.23V`

A

concentration of `H_2SO_4` remain constant, `H_2,O_2`

B

concentration of `H_2SO_4` remain constant, `O_2,H_2`

C

concentration of `H_2SO_4` remain constant, `O_2,H_2`

D

concentration of `H_2SO_4` remain constant, `S_2O_8^(2-),H_2`

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI|Exercise Level 1 (Q.1 To Q.30)|1 Videos

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI|Exercise Level 1 (Q.91 To Q.120)|1 Videos

  • DILUTE SOLUTION

    NARENDRA AWASTHI|Exercise Level 3 - Match The Column|1 Videos

  • GASEOUS STATE

    NARENDRA AWASTHI|Exercise Level 3 - Subjective Problems|1 Videos

Similar Questions

Explore conceptually related problems

An aqueous solution of Na_2SO_4 is electrolysed using Pt electrodes. The products at the cathode and anode are respectively:

when an aqueous solution of H_2SO_4 is electrolysed the product at anodes is :

When a solution of AgNO_3 (1 M) is electrolysed using platinum anode and copper cathode, what are the products obtained at two electrodes? Given : E_(cu^(2+)|cu)^(@)=+0.34 V , E_(H_2O|O_2,H^+)^(@)=-1.23 V E_(H^+|H_2)^(@)=+0.0V , E_(ag^+|Ag)^(@)=+0.8 V

E^(@) for Cl_2 (g) +2e^(-)to2Cl^- (aq) is 1.36 V , E^(@) for Cl^- (aq) to1//2Cl_2 (g) +e^- is:

Normality of 10V H_2O_2 is…………… .

In the expansion of (x +a)^n , the sums of the odd and the even terms are O and E respectively, prove that : O^2-E^2= (x^2-a^2)^n .

Complete the following chemical equation : MnO_4^(-)(aq) + S_2O_3^(2-)(aq)+ H_2O (l) rarr

In a hydrogen oxyge fuel cell, electricity is produced. In this process H_2 (g) is oxided at anode and O_2 (g) reduced at cathode Given: Cathode O_2(g)+2H_2O(l)+4e^(-)to4OH^(-)(aq) Anode H_2(g)+2OH^(-)(aq)to2H_2O(l)+2e^(-) 4.48 litre H_2 at 1atm and 273 k oxidised in 9650 sec. The current produced is (in amp):

In a hydrogen oxygen fuel cell, electricity is produced. In this process H_2 (g) is oxided at anode and O_2 (g) reduced at cathode Given: Cathode O_2(g)+2H_2O(l)+4e^(-)to4OH^(-)(aq) Anode H_2(g)+2OH^(-)(aq)to2H_2O(l)+2e^(-) 4.48 litre H_2 at 1atm and 273 k oxidised in 9650 sec. The mass of water produced is :

From the fllowing half-cell reactions and their standard potentials ,what is the smallest possible standard e.m.f for spontaneous reactions? PO_4^(3-)(aq)+2H_2O(l)+2e^(-)toHPO_3^(2-)+3OH^(-)(aq), E^(@)=-1.05V PbO_2(s)+H_2O(l)+2e^(-)toPbO(s)+2OH^(-)(aq),E^(@)=+0.28 V