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Wednesday, April 7, 2021

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Which half-reaction is most easily oxidized? Al3+ + 3e- Al = -1.66 V Cu2+ + 2e- Cu = 0.34 V Fe3+ + e- Fe2+ = 0.77 V Na+ + e- Na = -2.71 V Pb2+ + 2e- Pb = -0.13 VWhat must be done to the following half-reactions before they can be added together? Mn (s) → Mn 2+ (aq) + 2e − Fe 3+ (aq) + 3e − → Fe (s) Double the Mn half-reaction and triple the Fe half-reaction. Add H+ ions to the left-side of the Mn reaction. Triple the Mn half-reaction and double the Fe half-reaction. Double the Mn half-reaction.Consider the following half-reactions: (a) Based on E° values, which metal is the most easily oxidized? (b) Which metals on this list are capable of reducing Fe 2+ (aq) to Fe(s)? (c) Write a balanced chemical equation tor the reaction of Fe 2+ (aq) with Sn(s). Is this reaction product-favored or reactant-favored at equilibrium?5. List the metals in order of most easily oxidized first. Compare this order to that in Regents Table J. 6. Write balanced half reactions for the reduction of the halogens, F 2, Cl 2, Br 2, and I 2. List these in the order of most easily reduced first (you will need to refer to Regents Table J). 7.9.Which metal is most easily oxidized? A) 46.Write a balanced half-reaction equation for the oxidation that occurs in this operating cell. 47.State, in terms of the relative activity of metals, why the reaction in this cell occurs. 48.State, in terms of ions, how the porous barrier functions as a salt bridge in this cell.

Chem test 3 Ch 16 Flashcards | Quizlet

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. And remember, oxidation ALWAYS happens at the anode, and reduction ALWAYS happens at the cathode.When 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 was11.Which is the most easily reduced? A)Cl2 B)Br2 C)Hg2+ D)I2 E)I- 12.Which is the most easily oxidized? A)Cl- B)Br- C)Hg(l) D)I- E)Br2 13.Which is the strongest oxidizing agent? A)HNO3 B)Ag+ C)Cu D)H2 E)H+ 14.Which is the strongest reducing agent? A)Cl2 B)Br2 C)Cr D)Cr3+ E)Al 15.What is the oxidation potential for the reaction? Cu ®Cu2Consider 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).

Consider the following half-reactions: (a) Based on E

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.The electromotive series begins with the metal most easily oxidized, i.e., the metal with the greatest electron-donating tendency, and ends with the metal least easily oxidized. The tendency to be oxidized is not an absolute quantity; it can only be compared with the tendency of some other substance to be oxidized.Look on the LEFT side of the half-reactions for substances that are going to be reduced. Look on the RIGHT side to find substances that are going to be oxidized. Since Li is easy to oxidize, it is an excellent reducing agent (it reduces something else when it is oxidized).The potential of a half-reaction measured against the SHE under standard conditions is called the standard electrode potential for that half-reaction.In this example, the standard reduction potential for Zn 2 + (aq) Lithium metal is therefore the strongest reductant (most easily oxidized) of the alkali metals in aqueous solution. Note.To do that, identify the atoms which get reduced and get oxidized. Here are the two half-reactions from the above example: Ag +---> Ag Cu ---> Cu 2+ The silver is being reduced, its oxidation number going from +1 to zero. The copper's oxidation number went from zero to +2, so it was oxidized in the reaction. In order to figure out the half

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