Home
Class 12
PHYSICS
The atomic weight of silver and copper a...

The atomic weight of silver and copper are 108 and 64. A silver voltameter and a copper voltameter are connected in series and when current is passed `10.8` gm of silver is deposited. The mass of copper deposited will be

A

`6.4 gm`

B

`12.8 gm`

C

`3.2 gm`

D

`10.8 gm`

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Topper's Solved these Questions

  • HEATING AND CHEMICAL EFFECT OF CURRENT

    ERRORLESS |Exercise Heating Effect of Current|2 Videos

  • HEATING AND CHEMICAL EFFECT OF CURRENT

    ERRORLESS |Exercise Chemical Effect Current|1 Videos

  • ELECTROSTATICS

    ERRORLESS |Exercise Ordinary Thinking Objective Questions (Electric Flux and Gauss.s Law)|28 Videos

  • KINETIC THEORY OF GASES

    ERRORLESS |Exercise QUESTIONS|126 Videos

Similar Questions

Explore conceptually related problems

The current inside a copper voltameter

The chemical equivalent of copper and zinc are 32 and 108 respectively. When copper and silver voltameter are connected in series and electric current is passed through for sometimes, 1.6 g of copper is deposited. Then, the mass of silver deposited will be

A silver and zinc voltameter are connected in series and a current i is passed through them for a time t liberating W gm of zinc. The weight of silver deposited is nearly

A copper voltameter, a solver voltameter and a water voltamenter are connected in series and current is passed for some time. The ratio of the number of moles of copper, silver and hydrogen formed at the cathode is

The same current if passed through solution of silver nitrate and cupric salt connected in series. If the weights of silver deposited is 1.08g . Calculate the weight of copper deposited

A silver and a copper voltameter are connected in series with a 12.0 V battery of negligible resistance. It is found that 0.806g of silver is deposited in half an hour.Find (a) the mass of the copper deposited and (b) the energy supplied by the battery. ECE of silver = 1.12 xx 10^(-6) kg C^(-1) and that of copper = 6.6 xx 10^(-7) kg C^(-1)

Two electrolytic cells containing CuSO_(4) and AgNO_(3) respectively are connected in series and a current is passed through them until 1 mg of copper is deposited in the first cell. The amount of silver deposited in the second cell during this time is approximately [Atomic weights of copper and silver are respectively 63.57 and 107.88 ]

Three electrolytic cells A, B and C containing solutions of zinc sulphate, silver nitrate and copper sulphate, respectively are connected in series. A steady current of 1.5 ampere was passed through them until 1.45 g of silver were deposited at the cathode of cell B. How long did the current flow? What mass of copper and what mass of zinc were deposited in the concerned cells? (Atomic masses of Ag = 108, Zn = 65.4, Cu = 63.5)