ElectrochemistryHard
Question
Four moles of electrons were transferred from anode to cathode in an experiment on electrolysis of water. The total volume of the two gases (dry and at STP) produced will be approximately (in litres)
Options
A.22.4
B.44.8
C.67.2
D.89.4
Solution
At Cathode : 2H2O + 2e- → H2 + 2OH-] × 2
At Anode : 2H2O → O2 + 4H+ + 4e-
H2 = 2 mole
O2 = 1 mole Total volume = 3 × 22.4 = 67.2 L.
At Anode : 2H2O → O2 + 4H+ + 4e-
H2 = 2 mole
O2 = 1 mole Total volume = 3 × 22.4 = 67.2 L.
Create a free account to view solution
View Solution FreeMore Electrochemistry Questions
The molar conductivities ∧oNaOAc and ∧oHCl at infinite dilution in water at 25oC are 91.0 and 426.2 S cm2/mo...At 298K the standard free energy of formation of H2O(l) is -237.20 kJ/mole while ᐃGo of its ionisation into H+ ion...Which of the following substances: Na, Hg, S, Pt and graphite can be used as electrodes in electrolytic cells having aqu...The correct order of molar conductance at infinite dilution of LiCl, NaCl and KCl is...Ionic conductance at infinite dilution of A13+ and SO42− ions are 60 and 80 Ω−1 cm2 eq−1, respectively. The correct deta...