मराठी
महाराष्ट्र राज्य शिक्षण मंडळएचएससी विज्ञान (सामान्य) इयत्ता १२ वी

96500 Coulombs Correspond to the Charge on How Many Electrons?

Advertisements
Advertisements

प्रश्न

96500 coulombs correspond to the charge on how many electrons?

पर्याय

  • 1.6 X 1019

  • 6.022 X 1020

  • 6.022 X 1023

  • 6.022 X 1024

MCQ
Advertisements

उत्तर

6.022 x 1023

shaalaa.com
  या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?
2014-2015 (October)

APPEARS IN

व्हिडिओ ट्यूटोरियलVIEW ALL [1]

संबंधित प्रश्‍न

Number of faradays of electricity required to liberate 12 g of hydrogen is:


Suggest a list of metals that are extracted electrolytically.


Consider the reaction:

\[\ce{Cr2O^{2-}_7 + 14H+ + 6e- -> 2Cr^{3+} + 7H2O}\]

What is the quantity of electricity in coulombs needed to reduce 1 mol of  \[\ce{Cr2O^{2-}_7}\]?


How much charge is required for the following reduction?

1 mol of Al3+ to Al.


A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?


Three electrolytic cells A, B, C containing solutions of ZnSO4, AgNO3 and CuSO4, respectively, are connected in series. A steady current of 1.5 amperes 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?


State second law of electrolysis


Explain Faraday’s second law of electrolysis


Write the name of the cell which is generally used in transistors. Write the reactions taking place at the anode and the cathode of this cell.


Electrolytic cell uses electrical energy to bring about ____________.


According to Faraday’s First Law of Electrolysis, the amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the ____________.


In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?


What will happen during the electrolysis of aqueous solution of \[\ce{CuSO4}\] by using platinum electrodes?

(i) Copper will deposit at cathode.

(ii) Copper will deposit at anode.

(iii) Oxygen will be released at anode.

(iv) Copper will dissolve at anode.


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 or different? Explain your answer.


Assertion: Electrolysis of NaCl solution gives chlorine at anode instead of O2.

Reason: Formation of oxygen at anode requires overvoltage.


Consider the figure and answer the following question.

Cell ‘A’ has ECell = 2V and Cell ‘B’ has ECell = 1.1V which of the two cells ‘A’ or ‘B’ will act as an electrolytic cell. Which electrode reactions will occur in this cell?


Time Required to deposite one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium is


When during electrolysis of a solution of AgNO3, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be ______.


Given `1/a` = 0.5 CM–1, R = 50 ohm, N = 1.0 then equivalent conductance of electrolytic cell is


On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be ______.


The quantity of electricity needed to separately electrolyse 1 M solution of ZnSO4, AlCl3, and AgNO3 completely is in the ratio of ______.


Through an aqueous solution of an unknown salt of metal M (M = 200 g/mol) a current of 1.93 A is passed for 50 min. If 4 g of metal is produced at cathode. The charge on metal ion in solution is ______.


A current of 4 amp was passed for 2 hours through a solution of copper sulphate when 5.0 g of copper was deposited. The current efficiency is ______% (Cu = 63.5).


On passing electricity through nitrobenzene solution, it is converted into azobenzene. The mass of azobenzene is ______ mg, if the same quantity of electricity produces oxygen just sufficient to burn 96 mg of fullerene (C60


Assertion (A): During electrolysis of aqueous copper sulphate solution using copper electrodes hydrogen gas is released at the cathode.

Reason (R): The electrode potential of Cu2+/Cu is greater than that of H+/H2.

Select the most appropriate answer from the options given below:


How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten Al2O3?

(Given: Molar mass of Aluminium is 27 g mol−1.)


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×