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Which half-reaction is most easily oxidized?
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Electrochemistry | Chemistry for Non-Majors – The elements at the top are the easiest to oxidize, while those at the bottom are the most difficult to oxidize. The Table below shows the activity series together with each element's oxidation half-reaction. Notice that zinc is listed above copper on the activity series, which means that zinc is more easily oxidized than copper.Table 4.5 gives the activity series in aqueous solution for many of the most common metals. Hydrogen is also included in the table. The metals at the top of the table are most easily oxidized; that is, they react most readily to form compounds. Notice that the alkali metals and alkaline earth metals are at the top. They are called the activeDetermine 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. And remember, oxidation ALWAYS happens at the anode, and reduction ALWAYS happens at the cathode.
Chemistry: The Central Science, Chapter 4, Section 4 – True or false: Metals at the bottom of the activity series are most easily oxidized. False, at the top. Oxidation half-reaction: S2O3^2- (aq) + 5 H2O (l) 2 SO4^2- (aq) + 10 H+ (aq) + 8e-2. Multiply the reduction half reaction by 4 to balance electrons between the 2 half reactions.The element that gets oxidized will be on the product side of the half reaction The most easily oxidized are at the bottom of the table on the right hand side (product side) Li (s) is the most easily oxidized element on the table. Rules for Spontaneous Rxns and the ½ Rxn Table Substances to the left and those below them on the right reactWhen copper oxidized to form this patina layer, the copper atoms became copper (II) ions (Cu 2+). Write a balanced half-reaction for this oxidation of copper. 81. Where the iron framework came in contact with the copper surface, a reaction occurred in which iron was oxidized. Using information from Reference Table J, explain why the iron was
How do I do determine which half-reaction is at the – If we have a higher (positive) potential the compound would be more inclined to a reduction and vice-versa if we have a smaller potential (negative) the compound would be more inclined to oxidation. In this case, the most negative value is for Na+, so this atom would be more easily oxidized.Iodide ion, I- , is one of the most easily oxidized species. Balance each of the following oxidation-reduction reactions, which take place in acidic solution, by using the "half-reaction" method. a. IO 3 − ( aq ) + I − ( aq ) → I 2 ( aq ) b.Consider the following half-reactions: Based on E degree values, which metal is the most easily oxidized? Which metals on this list are capable of reducing Fe2+(aq) to Fe(s)? Write a balanced chemical equation for the reaction of Fe2*(aq) with Sn(s).