Calculate the quantity of electricity required to deposit 0.09 g of Aluminium during the following electrode reaction. `Al^(3+) + 3e^- rarr Al`.

In a classroom, the teacher has explained the quantitative aspects of electrolysis by stating the Faraday's laws of electrolysis. Calculate the quantity of electricity required to deposit 0.09 g of aluminium during the following electrode reaction: Al^3 + 3e^(-) to Al ( Al=27u)

The amount of electricity required to deposit 1 mole of aluminium from a solution of A Cl_3 will be

Complete the following reactions? '4Al+3O_2

Complete the following ionic equations : Al^(3+)+3e^(-)rarr ……….

Calculate the quantity of electricity that would be required to reduce 12.3 gm of nitrobenzene to aniline if current efficiency is 50%

Calculate the quantity of electricity that will be required to liberate 710g of Cl , gas by electrolysing a conc. solution of NaCl . What is the amount of NaOH and volume.of H_2 at 27^circ C and 1 atm pressure is obtained during this process?

Disuss the change in hybridisation of Al atom in the following reaction AlCl_3+Cl^1 rarr AlCl_4^-

Complete the following reactions: CH_3-CH = CH_2 + HCl rarr

Describe the change in hybridisation (if any) of the Al atom in the following reaction. 'AlCl_3+Cl^- rarr AlCl_4^-'

Calculate the standard cell potentials of galvanic cell. Also calculate Delta G^0 and equilibrium constant of the following cell, reaction. Fe^(2+)(aq)+Ag^+(aq) rarr Fe^(3+)(aq)+Ag(s) E^0 Ag^+I Ag =0.80V,E^0 Fe^(3+)IFe^(2+)=0.77V .