The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of `PbSO_(4)` electrolyzed g during the process is: (Molar mass of `PbSO_(4) = gmol^(-1)`)

The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO_(4) electrolyzed in g during the process is : (Molar mass of PbSO_(4)=303gmol^(-1) )

The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO_(4) electrolyzed in g during the process is : (Molar mass of PbSO_(4)=303gmol^(-1) )

The anodic half-cell of lead-acid battery is recharged using electricity of 6 Faraday. The amount of PbSo_(4) electrolyzed in moles during the process is__________.

The anodic half-cell of lead-acid battery is recharged using electricity of 6 Faraday. The amount of PbSo_(4) electrolyzed in moles during the process is__________.

In a lead-acid battery, if 1 A current is passed to charge the battery for 1 h, what is the amount of PbSO_(4) converted to PbO_(2) ? (Given data 1 F=96500 C mol^(-1))

0.02F current is drawn from a lead storage battery. Change in the mass of H_2SO_4 and PbSO_4 are (mol. mass of PbSO_4 =303 gmol^(−1) ):

Calculate the number of electrons in a small, electrically neutral silver pin that has a mass of 10.0 g . Silver has 47 electrins per atom, and its molar mass is 107.87 gmol^(-1) .

Calculate the number of electrons in a small, electrically neutral silver pin that has a mass of 10.0 g . Silver has 47 electrins per atom, and its molar mass is 107.87 gmol^(-1) .