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 ENGLISH|Exercise LEVEL-2|28 Videos

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI ENGLISH|Exercise LEVEL-3|37 Videos

  • DILUTE SOLUTION

    NARENDRA AWASTHI ENGLISH|Exercise leval-03|23 Videos

  • GASEOUS STATE

    NARENDRA AWASTHI ENGLISH|Exercise Subjective problems|15 Videos

Similar Questions

Explore conceptually related problems

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 Pt anode and Cu cathode, the products at two electrodes are? E_(cu^(2+)|cu)^(@)=+0.34 "V" , E_(O_2,H^+|H_2O)^(@)=+1.23"V",E_(ag^+|Ag)^(@)=+0.8 "V"

Given below are a set of half-cell reactions (acidic medium) along with their E_(@) with respect to normal hydrogen electrode values. Using the data obtain the correct explanation to question given below. {:(I_(2)+2e^(-)rarr2I^(-),E^(@)=0.54),(Cl_(2)+2e^(-)rarr2Cl^(-),E^(@)=1.36),(Mn^(2+)+e^(-)rarrMn^(2+),E^(@)=1.50),(Fe^(3+)+e^(-)rarrFe^(2+),E^(@)=0.77),(O_(2)+4H^(+)+4e^(-)rarr2H_(2)O,E^(@)=1.23):} Among the following, identify the correct statement:

Given below are a set of half-cell reactions (acidic medium) along with their E_(@) with respect to normal hydrogen electrode values. Using the data obtain the correct explanation to question given below. {:(I_(2)+2e^(-)rarr2I^(-),E^(@)=0.54),(Cl_(2)+2e^(-)rarr2Cl^(-),E^(@)=1.36),(Mn^(2+)+e^(-)rarrMn^(2+),E^(@)=1.50),(Fe^(3+)+e^(-)rarrFe^(2+),E^(@)=0.77),(O_(2)+4H^(+)+4e^(-)rarr2H_(2)O,E^(@)=1.23):} While Fe^(2+) is stable, Mn^(3+) is not stable in acid solution because:

Role of SO_2 in the following reaction respectively are, (a) Fe_2(SO_4)_3 + SO_2 +2H_2O rarr 2FeSO_4 + H_2SO_4 , (b) 2H_2S + SO_2 rarr 2H_2O + 3S

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 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 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

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. If current produced in fuel cell, is used for the deposition of Cu^(+2) in 1L,2M CuSO_4 (aq) solution for 241.25 sec using Pt. electrode, the pH of solution after electrolysis is:

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reaction and their standard potentials are given below: MnO_(4)^(-)(aq) +8H^(+)(aq) +5e^(-) rarr Mn^(2+)(aq) +4H_(2)O(l) E^(@) = 1.51V Cr_(2)O_(7)^(2-)(aq) +14H^(+) (aq) +6e^(-) rarr 2Cr^(3+)(aq) +7H_(2)O(l), E^(@) = 1.38V Fe^(3+) (aq) +e^(-) rarr Fe^(2+) (aq), E^(@) = 0.77V CI_(2)(g) +2e^(-) rarr 2CI^(-)(aq), E^(@) = 1.40V Identify the only correct statement regarding quantitative estimation of aqueous Fe(NO_(3))_(2)