The fundamental electronic charge of water will be determined.
A system of collecting the formation of H2 and O2 using two inverted glass collections tubes and a 1-L beaker filled with water will be setup. An electrolyte (H2SO4) will be added to water to make it an electrical conductor. A small amount of electricity will be applied to the water (roughly 400 mA) to oxidize the oxygen and reduce the hydrogen at the same time. The molecular hydrogen and oxygen gases produced will be trapped in the separated, inverted tubes so that their volumes can be measured.
In comparing the volume of gases produced, applying Dalton’s Law and the Ideal Gas Equation along with the application of the stoichiometric ratio between the electron and the gases, the fundamental electronic charge will be determined.
H+ ions will join together at the cathode (the negative electrode) to produce H Atoms, and the H atoms will join to form molecules of H2 gas. At the positive electrode (the anode), H20 molecules will decompose to replace the H+ ions lost and release O2 gas. The reactions appear below.
2H+(aq) + 2e- ---> H2(g) Reduction (at the cathode) 2H20(l) ---> 4H+(aq) + O2(g) + 4e-Oxidation (at the anode)
The volume of H2 and O2 will be directly proportional to the time and current applied to the system. This will provide the number of electrons consumed on a stoichiometric ratio as follows:
1 H2(g) to 2 e-Reduction (at the cathode)(1)
1 O2(g) to 4 e-Oxidation (at the anode)(2)
The moles of electrons can be expressed as a rearrangement of the Ideal Gas Equation: Ne = PV/RT(3)
Where P = pressure in atm, V = volume in L, R = Gas Constant of 0.08206 atm mol-1 K-1 and T = temperature in Kelvin
The actual electronic charge of water will be calculated as follows:
e- = it/NeNx the stoichiometric ratio (1) or (2) above