Table of standard electrode potentials
-Using a table of standard electrode potentials decide which of the following statements is completely true.(Note that some imaginary elements are being used in these questions).

Question

Table of standard electrode potentials 
-Using a table of standard electrode potentials decide which of the following statements is completely true.(Note that some imaginary elements are being used in these questions).

Quizplus · Accepted Answer

Additional information for each answer choice: A: If Nt²⁺ can oxidize Cu²⁺, then the potential to reduce Ni²⁺ must be greater than the reduction potential for Cu²⁺. But the key to this problem is to realize that oxidation of Cu²⁺ would require the additional loss of electrons from Cu²⁺, which is difficult (there is no listed equation for this for that reason). Therefore Ni²⁺ will not oxidize Cu²⁺A similar argument can be made for Al³⁺. For Al³⁺ to reduce H⁺, it must be oxidized, which would again require loss of electrons from a highly charged species. B: Br₂ can oxidize Nt, as the reduction potential of Br₂ is higher than Ni in the reduction table. If you calculated the reduction potential for this, you would get a positive value.If the second part was correct, H₂ can reduce Cl^-, then you would be reducing Cl^-, which would result in a Cl^-², and that is not a favorable process (not on table). C: Cu²⁺ can oxidize H₂as the reduction potential for Cu²⁺ is higher than that for H₂ on the table (hydrogen is a value of zero). Ni can also reduce Cl₂, because the reduction potential of Cl₂ is larger than that of Nt.One key for this type of problem is to write out the half reaction that refers to the oxidation or reduction process mentioned and see if you can compare the potentials for these equations if possible. If the reduction potential is not available, you need to logically ask if the process would be easy to do or not.

Table of Standard Electrode Potentials