Na-amalgam is prepared by electrolysis of `NaCl` solution using liquid Hg as cathode. How long should the current of 10 amp. Is passed to produce `10%` Na-Hg on a cathode of 10 gm Hg. (atomic mass of `Na=23`).
(A). 7.77 min
(B). 9.44 min.
(C). 5.24 min.
(D). 11.39 min

Na- amalgam is prepared by electrolysis of NaCl solution using liquid Hg as cathode . How long should the current of 10 amp . Is passed to produce 10% Na-Hg on a cathode of 10gm Hg . ( atomic mass of Na=23) .

Cd amalgam is preapred by electrolysis of a solution CdCI_(2) using a mercury cathode. How long should a current of 5A be passed in order to prepare 12% Cd-Hg amalgam on a cathode of 2g, Hg ( atomic weight of Cd = 112.4)

Cadmium amalgam is prepared by electrolysis of a sodium of CdCl_2 using a mercury cathode. How long should a current of 4 A be passed in order to prepare 10% by mass Cd in Cd-Hg amalgam on cathode of 4.5 g Hg? (atomic mass of Cd=112)

Na-Amalgam is prepared by electrolysis of aq. NaCI solution using 10gm Hg cathode. How many Faraday's of electricity is required to prepare 18.7% Na-Amalgam (current Eff = 50%)

Zn amalgam is prepared by elctrtolysis of aqueous ZnCI_(2) using 9 gram Hg cathode how much current is to be pased through ZnCI_(2) solution for 1000 seconds to prepare a Zn amalagam with 25% by weight ? (atomic masss Zn =65.4 g)

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 4.0M aqueous solution of NaCl is prepared and 500mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes ( atomic mass of Na is 23 and Hg is 200)(1F=96500C) . The total charge ( coulomb ) required for complete electrolysis is (a)24125 (b)48250 (c)96500 (d)193000

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10mA current. The time required to liberate 0.01mol of H_(2) gas at the cathode is (1F=96500C mol ^(-1)) (a) 9.65xx10^(4)s (b) 19.3xx10^(4)s (c) 28.95xx10^(4)s (d) 38.6xx10^(4)s

A 2.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: Na = 23, Hg = 200, 1 faraday = 96500 coulomb). If the cathode is a Hg electrode, the maximum weight (in gram) of amalgam formed from this solution is

Chemical reactions involve interaction of atoms and molecules. A large number of atoms and molecules (approximately 6.022 xx 10^(23) ) are present in a few grams of any chemical compound varying with their atomic/molecular masses. To handle such a large number conveniently, the mole concept was introduced. This concept has implications in diverse areas such as analytical chemistry, biochemistry, electrochemistry adn radiochemistry. The following examples illustrate a typical case involving chemical/electrochemical reaction which requires a clear understanding of mole concept. A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of the solution is electrolysed. This lead to the evolution of chlorine gas at one of electrodes (atomis mass : Na = 23 , Hg = 200 , 1F = 96500 C) If the cathode is a Hg electrode, the maximum weight (g) of amalgam formed from the solution is :