Home
Class 12
CHEMISTRY
1000 ml 2 M CuSO(4) is electolysed by a ...

1000 ml 2 M `CuSO_(4)` is electolysed by a current of 9.65 amp for 2 hours. Which is //are correct?

A

afterelectrolysis remaining concentration of `Cu^(+2)` is 1.64 M using Cu electrode

B

After electrolysis remaining concentratin of `Cu^(+2)` is 1.64 M using Pt electrode

C

When remaining coincentration of `Cu^(+2)` is 1.822 M then volume of solution is reduced by 10% using Pt electrode

D

17.15 gm copper deposit when current efficiency is 75% using copper electrode

Text Solution

AI Generated Solution

Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (SECTION D) Linked Comprehension Type Questions|6 Videos

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (SECTION E) Assertion - Reason Type Questions|10 Videos

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (SECTION B) Objective Type Questions (One option is correct)|25 Videos

  • COORDINATION COMPOUNDS

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (Section-J Aakash Challenger Questions )|10 Videos

  • ENVIRONMENTAL CHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT (SECTION-D) (Assertion - Reason Type Questions)|4 Videos

Similar Questions

Explore conceptually related problems

1000mL 1M CuSO_4 (aq) is electrolysed by 9.65 A current for 100 sec using Pt-electrode which is /are correct statements?

100mL of 1M solution of CuBr_(2) was electrolyzed with a current of 0.965 ampere hour. What is the normality of the remaining CuBr_(2) solution ? a. 1.64" "b.3.28" "c.0.82" "d.4.92

100 ml, 0.05 M CuSO_4 solution is electrolysed by using current of 0.965 Å for 100 min.Find the pH of solution at the end of electrolysis.

How many gram of copper metal will be deposited when a solution of copper sulphate (CuSO_4) is electrolysed with a current of 9.65 ampere for 10 minutes? (1F = 96500 C, Atomic mass of Cu = 63.5 u)

50mL of 0.1M CuSO_(4) solution is electrolysed with a current of 0.965A for a period of 200sec. The reactions at electrodes are: Cathode: Cu^(2+) +2e^(-) rarr Cu(s) Anode: 2H_(2)O rarr O_(2) +4H^(+) +4e . Assuming no change in volume during electrolysis, calculate the molar concentration of Cu^(2+),H^(+) and SO_(4)^(2-) at the end of electrolysis.

500 ml CuSO_(4) solution was electrolysed using a current of 2 amp (efficiency =75%) for 60 min calculate the pH of solution at the end of electrolysis (Assume initial pH=7)

In the electrolysis of 7.2L aqueous solution of CuSO_(4) , a current of 9.65A passed for 2 hours. Find the weight of Cu deposited at cathode.

Calculate volume of the gases liberated at STP if 1 L of 0.2 molar solution of CuSO_(4) is electrolysed by 5.79 A current for 10000 seconds.

In CuSO_(4) · 5H_(2)O

CuSO_(4).5H_(2)O is blue in colour because