In the electrolysis of dilute sulfuric acid using inert electrodes, oxygen gas is produced at the positive electrode (anode) according to the half-equation:
2H2O(l)→O2(g)+4H+(aq)+4e− 2\text{H}_2\text{O}(l) \to \text{O}_2(g) + 4\text{H}^+(aq) + 4\text{e}^- 2H2O(l)→O2(g)+4H+(aq)+4e−Suggest a suitable element that can be used as an inert electrode in this process.
The volume of oxygen gas collected at the anode is often slightly less than the expected volume, even though there are no leaks in the apparatus. Suggest an explanation for this observation.
During an electrolysis experiment, a total of 57 900 coulombs57\,900\text{ coulombs}57900 coulombs of electric charge was passed through the solution. Calculate the amount, in moles, of oxygen gas (O2\text{O}_2O2) formed.
[One faraday = 96 500 coulombs96\,500\text{ coulombs}96500 coulombs]
