330238 How many Faradays of electricity is required to produce 4.8 g of Mg at cathode in the electrolysis of molten MgCl2
Electrode reaction:Mg2++2e−→Mg(s)To produce 24g of Mg from molten MgCl2.electricity required = 2FTo produce 4.8 g Mg from MgCl2, electricity required=(2F)×4.8g24g=0.4F
330239 The electrochemical equivalent of a metal is “x” gcoulomb−1. The eq. wt of metal is
E=x×96500
330258 If an aqueous NaCl solution is electrolysed using a current of 5 A for 200 min. Volume of Cl2( g) in litres produced under STP condition is (F=96000C).
I=5At=200min=200×60sec.Equivalent volume of Cl2;Ve=11.2 LV=It⋅Ve96500=5×200×60×11.296500V=6.96L≈7L
330259 How many Faradays of electricity are required to oxidize 1 mol of water to dioxygen?
H2O⟶2H++2e−+12O2Hence, for the oxidation of one mole of water to dioxygen, 2 moles of electrons =2 F electricity is required.
330260 Which one of the following statements is correct for electrolysis of brine solution?
Statement 4 is incorrect. H2 is formed at cathode .NaCl(aq)→Na++Cl−Cathode reaction:2H2O+2e−→ reduction H2( g)+2OH−Anode reaction :2Cl−→ reduction Cl2( g)+2e−