The first thing to do is to work out how many coulombs of electricity flowed during the electrolysis. Faraday's laws of electrolysis predicts the amount of substance altered at the electrode due to the electricity that is transferred at the electrode. We have just used that without actually stating it - it is basically obvious! } catch (ignore) { } For calculation purposes, we need to know how to relate the number of moles of electrons which flow to the measured quantity of electricity. try { Calculate the volume of hydrogen produced (measured at room temperature and pressure - rtp) during the electrolysis of dilute sulphuric acid if you use a current of 1.0 amp for 15 minutes. engcalc.setupWorksheetButtons(); You will need to use the BACK BUTTON on your browser to come back here afterwards. The quantities of substances produced or consumed The mass of the substance liberated at an electrode, The total electric charge passed through the substance, The valency number of ions of the substance (electrons transferred per ion). This value is known as the Faraday constant. 1 mol of electrons is 1 faraday. Add to Solver. }); You may come across the formula F = Le, where F is the Faraday constant, L is the Avogadro constant and e is the charge on an electron (in terms of the number of coulombs it carries). That means the 1 mole of electrons must carry. Convert the moles of electrons into coulombs of charge. F = 9.65 x 104 C mol-1 (or 96500 C mol-1). Use of these equations are illustrated in the following sections. window.jQuery || document.write('