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This is the second of our many quizzes on Half-reactions. Click on this to access more such competitive quizzes on Physical Chemistry.

Half-reactions Quiz 2

chemistry

 Positive electrode potential of a half cell reaction describes:

 Reduction potential of a half-cell reaction is generally positive.

 Atoms with more positive value of reduction potential shows reduction property more efficiently.

 If half-cell reaction of a redox reaction, it is given as ${\text{A}} \to {{\text{A}}^{{\text{2 + }}}}{\text{ + 2}}{{\text{e}}^{\text{ - }}}$, then identity what it defines: <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/83f30ee0-5fc4-4245-a6ac-32a44a93cf289187354139888019052.png"/>

   Half-cell reactions define either oxidation or reduction.

In the above given reaction species A removes two electrons and this is the property of oxidation reaction. So the above half-cell reaction is an oxidation reaction.

  Half-cell reaction is useful in which section of chemistry:

 Half-cell reaction defines the electrode potentials of electrodes present in a cell.

 Half-cell reaction is used to define the properties of cell reactions, so it is useful in the Electrochemistry section of chemistry.

 Half-cell reaction gives knowledge about the exchange of electrons.

Exchange of electrons efficiently is shown by metals, so half-cell reaction is used to write for metals.

 If - 2.85 and - 5.5 are two negative electrode potentials of two different electrodes, then which one have more reducing ability then other:

 In the above two values - 2.85 is slightly positive as compared to the - 5. 5 which is more negative. So electrodes with - 2.85 value have more reducing ability than others.