Therefore, since we would normally expect halogens to have become reduced (to halides), the halide is actually oxidized (to the halogen), while the metal cation is reduced to the metal element. « Reply 1 on: December 15, 2008, 02:25:49 PM » yes correct for electrolysis of molten calcium chloride. (The cathode is on the left, and the anode is on the right.) The anode reaction is 2Cl-> Cl2 (g) + 2e- and the cathode reaction is Ca2+ + 2 e-> Ca(s) Is this correct, or have I mixed these up. Take this image and replace #"Pb"# with #"Ni"# and you'll have a representation of this process: This is going to correspond to the nonintuitive result, the result backwards from the spontaneous process. Next, it is important to note that electrolysis forces a nonspontaneous process to occur by running electricity through it. For the electrolysis of 2E required to drive this reaction. So, the two reduction half-reactions so far are:Īgain, the reduction has it so that the atoms gain electrons. Since you are looking at #"NiBr"_2(l)#, it will split into #"Ni"^(2+)# and #2"Br"^(-)#, since halides have charges of #-1# as outer atoms, and the nickel ion will make up the remaining positive charge such that #2 + (-1 xx 2) = 0#, for a neutral compound. Therefore, we should begin by writing the preliminary half-reactions for the reduction of nonmetals and metal cations. Electric current among ions is due to the movement of electrons. Similarly, electrolysis of molten solids will produce their ions as PURE LIQUIDS and induce flow of electric current. The loss in weight of anode is equal to gain in weight of cathode. Anode: Cu(s) Cu ++ + 2e Cathode: Cu ++ (aq) + 2e Cu (s). Explanation: During electrolysis of CuSO 4 solution using Cu electrodes, the cell reaction is.
When you melt a solid into a liquid and then electrolyze it, notice the similarity to the word "electrolyte".Įlectrolytes conduct electricity, and that is because they are ions that when placed into aqueous solution can carry and thus conduct electric charge with them. The correct option: (d) 2 gram of copper goes into solution as Cu 2+.
Determine which half-reaction should be reversed based on which ion should be reduced or oxidized more easily, keeping in mind that the backwards (nonspontaneous) reaction to what you expect will be made to occur.Īnd remember, oxidation ALWAYS happens at the anode, and reduction ALWAYS happens at the cathode.
Write the reduction half-reactions that turn the neutral element into its ion by adding electron(s).Determine what ions came from the compound.
0 kommentar(er)
