Home
Class 12
CHEMISTRY
A solution of CuSO(4) is electroysed for...

A solution of `CuSO_(4)` is electroysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ?
(Molar mass of `Cu=63.5 g//mol)`

Text Solution

AI Generated Solution

To find the mass of copper deposited at the cathode during the electrolysis of a copper sulfate solution, we can follow these steps: ### Step 1: Convert time from minutes to seconds Given that the electrolysis occurs for 10 minutes, we need to convert this time into seconds: \[ \text{Time (T)} = 10 \text{ minutes} \times 60 \text{ seconds/minute} = 600 \text{ seconds} \] ...
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise Try Yourself|19 Videos

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (SECTION A) Objective Type Questions (One option is correct)|43 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

A solution of CuSO_(4) is electrolyzed for 10 min with a current of 1.5A . What is the mass of Cu deposited at the cathode? [ Atomic mass of Cu=63g]

A solution of Ni(NO_(3))_(2) is electrolyzed between platinum electrodes using a current of 5 amperes for 20 min. What mass of Ni is deposited at the cathode? (Atomic mass of Ni = 58.7) [Report your answer by rounding it upto nearset whole number]

A solution of Ni(NO_(3))_(2) is electrolyzed between platium electrodes using a current of 5A for 20 mi n . What mass of Ni is deposited at the cathode ?

Two faraday of electricity is passed through a solution of CuSO_(4) . The mass of copper deposited at the cathode is: (at mass of Cu = 63.5 amu)

Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same of different? Explain your answer.

Three electrolytic celss A,B,C containing solutions of ZnSO_(4),AgNO_(3) and CuSO_(4) , respectively are connected in series. A steady current of 1.5 amperes was passes through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow ? What mass of copper and zinc were deposited.

The mass of 0.4 mol Ar is 16 g. What is the molar mass of Ar atoms?

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)

Three electrolytic cell A,B , and C contaning solutions of ZnSO_(4), AgNO_(3) , and CuSO_(4) , respectively, are connected in series. A steady current of 1.5A was passed through them until 1.45 g of silver deposited at the cathode of cell B . How long did the current flow ? What mass of copper and zinc were deposited ?

2.5 amperes of current is passed through copper sulphate solution for 30 minutes. Calculate the number of copper atoms deposited at the cathode (Cu = 63.54).