Home
Class 11
CHEMISTRY
What is the potential of an electrode wh...

What is the potential of an electrode which originally contained 0.1 `MNO_3^-)` and `0.4MH^+` and which has been treated by 80% of the cadmium necessary to reduce all the `NO_3^-` to NO(g) at 1 bar?
Give: `NO_3^(-)+4H^++3e^-)to NO+2H_2O, E^(@)=0.96V, log2=0.3`

A

0.84V

B

1.08V

C

1.23V

D

1.36V

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI|Exercise Level 3 - Passage|5 Videos

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI|Exercise Level 3 - One Or More Answers Are Correct|3 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

The standard reduction potential for the half cell: NO_3^- (aq)+2H^+ (aq)+barerarrNO_2+H_2O is 0.78v. What will be the reduction of the half cell in a neutral solution? Assume all the other species to be at unit concentration.

For a cell reaction 2H_2(g)+O_2(g)to2H_2O(l)/_\_rS_(198)^(@)=-0.32KJ//k . What is the value of /_\_fH_(298)^(@)(H_2O,l) ? Given: O_2(g)+4H^+(aq)+4e^-)to2H_2O(l), E^(@)=1.23V

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

W is the mass of iron (in g) which will be converted into Fe_(3)O_(4) by the action of 18 g of steam on it . What is the value of W/7 ? Fe+H_(2)O to Fe_(3)O_(4)+H_(2)

The mass of a mixture containing HCI and H_2 SO_4 is 0.1g On treatment with an excess of an AgNO_3 solution , reacted with this acid mixture given 0.1435g of AgCI . Mass % of the H_2SO_4 mixture is :

Calculate the molarity of each of the following soluton: 30g of CO(NO_3)_2. 6H_2O in 4.3 L of solution.

The Van't Hoff factor for 0.1 M Ba(NO_3)_2 solution is 2.74. the degree of dissociation is

Calculated the molarity of each of the following solutions: (a) 30 g of Co(NO_3)_2 . 6H_2O in 4.3 L of solution (b) 30ml of 0.5 M H_2SO_4 diluted to 500 mL.

Calculate the potential for half cell containing 0.1 M K_2Cr_2O_7(aq) , 0.20 M Cr^(3+)(aq) and 1.0xx10^-4 M H^(+)(aq) The half cell reaction is. CrO_7^(2-)(aq)+14H^(+)+6barerarr2Cr^(3+)(aq)+7H_2O(l) and the standard electrode potential is given as: E^@=1.33V .

STATEMENT-1: 0.1 MH_(3)PO_(3) (aq) solution has normality equal to 0.3 N when completely reacted with NaOH. STATEMENT-2 : H_(3)PO_(3) is a dibasic acid.