91影视

The electrolysis of brine involves two simultaneous half-reactions, one occurring at the anode (positive electrode) and the other, at the cathode (negative electrode). At the anode, chloride ions (Cl鈦�) are oxidized to chlorine gas (Cl鈧�). The oxidation half-reaction is: 2 Cl鈦�(aq) 鈫� Cl鈧�(g) + 2 e鈦� At the cathode, water molecules (H鈧侽) are reduced to produce hydrogen gas (H鈧�) and hydroxide ions (OH鈦�). The reduction half-reaction is: 2 H鈧侽(l) + 2 e鈦� 鈫� H鈧�(g) + 2 OH鈦�(aq)

Since both half-reactions involve 2 moles of electrons, they can be combined directly. Adding the two half-reactions together gives the overall balanced chemical equation for the electrolysis of aqueous sodium chloride: 2 Cl鈦�(aq) + 2 H鈧侽(l) 鈫� Cl鈧�(g) + H鈧�(g) + 2 OH鈦�(aq) However, since we started with sodium chloride (NaCl), we should include it in the equation. The sodium ions (Na鈦�) present in brine combine with the hydroxide ions (OH鈦�) produced at the cathode to form sodium hydroxide (NaOH). Now, the balanced equation becomes: 2 NaCl(aq) + 2 H鈧侽(l) 鈫� Cl鈧�(g) + H鈧�(g) + 2 NaOH(aq) This balanced equation describes the overall process of the electrolysis of aqueous sodium chloride, resulting in the production of chlorine gas, hydrogen gas, and sodium hydroxide.