Home
Class 12
CHEMISTRY
Electrolysis of dilute aqueous NaCl solu...

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10mA current. The time required to liberate 0.01 mole of `H_(2)` gas at the cathode is ( 1F = 96500 C `"mol"^(-1)` )

A

`9.65xx10^(4)` s

B

`19.3 xx 10^(4)s`

C

`28.95 xx 10^(4) s`

D

`38.6 xx 10^(4) s`

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise QUESTIONS FOR ASSESSMENT ( PART 1 )( VERY SHORT ANSWER TYPES QUESTIONS) |7 Videos

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise QUESTIONS FOR ASSESSMENT ( PART 1 )( SHORT ANSWER TYPES I QUESTIONS) |1 Videos

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise QUESTIONS FOR PRACTICE (PART 1) ( CONDUCTOR ELECTROLYTES AND THEIR DISSOCIATION, ELECTROLYSIS, ITS LAW AND APPLICATIONS)( LONG ANSWER TYPE QUESTIONS) |8 Videos

  • D-BLOCK ELEMENTS

    ARIHANT PUBLICATION|Exercise Chapter practice (Long answer type questions)|2 Videos

  • ELEMENTS : NITROGEN FAMILY

    ARIHANT PUBLICATION|Exercise CHAPTER PRACTICE ( Long Answer Type Questions ) |11 Videos

Similar Questions

Explore conceptually related problems

State and explain laws of electrolysis. How much current in ampere is required to liberate H_2 gas at the rate of 1ml/sec at NTP from HCl solution ?

Calculate the strength of the current required to deposit 1.2 g of magnesium from molten MgCl_(2) in 1h. [ 1F = 96500 C "mol"^(-1) , Atomic mass of Mg = 24.0 ]

An aqueous solution of copper sulphate, CuSO_(4) was electrolysed between platinum electrodes using a current of 0.1287 A for 50 min. [ Given atomic mass of Cu = 63. 5 g "mol"^(-1) ] ( i) Write the cathodic reaction. (ii ) Calculate (a) electric charge passed during electrolysis. (b) mass of copper deposited at the cathode. [ Given, 1 F = 96500 C " mol"^(-1) ]

An aqueous solution contains a substance which yields 4 xx 10^-3 mol liter^-1 ion of H_3O^+ . If log 2 = 0.3010 the pH of the solution is:

The electrolysis of hydrochloric acid results in the formation of 1 gm equivalent of H_2 gas at the cathode. The weight of Cl_2 liberated at anode is

The boiling point of an aqueous solution of a nonvolatile solute is 100.15^@C. What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The value of K_b and K_f for water are 0.512^@C and 1.86^@C K molality^-1:

Silver is electrolytically deposited on a metallic vessel of total surface area 900 c m^(2) by passing a current of 0.5A for 2h. Calculate the thickness of silver deposited . Given, density of silver =10.5 g c m^(-1) . Atomic mass of silver = 108u, F = 96500 C "mol"^(-1)

Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid were connected in a series. A steady current of 2.5 A was passed through them till 1.078 g of silver was deposited ( Ag = 107.8 g //" mol" ) (a) How much electricity was consumed? (b) What is the weight of oxygen gas liberated during the reaction?

ARIHANT PUBLICATION-ELECTROCHEMISTRY-QUESTIONS FOR ASSESSMENT ( PART 1 CONDUCTORS , ELECTROLYTES AND THEIR DISSOCIATION, ELECTROLYSIS , ITS LAWS AND APPLICATIONS) ( MULTIPLE CHOICE TYPE QUESTIONS)
  1. Electrolysis of dilute aqueous NaCl solution was carried out by passin...

    Text Solution

    |

  2. How many Coulomb of electricity are required for the oxidation of one ...

    Text Solution

    |

  3. How many Faradays of electricity are required to deposit 10 g of calci...

    Text Solution

    |