Which of the following reactions would be classified as oxidation-reduction?
Oxidation-reduction reactions, also known as redox reactions, are a fundamental class of chemical reactions that involve the transfer of electrons between reactants. These reactions are crucial in various natural processes, such as cellular respiration and photosynthesis, as well as in industrial applications, such as electroplating and metal refining. In this article, we will explore several examples of oxidation-reduction reactions and determine which among them fit the criteria for this classification.
One of the most common examples of an oxidation-reduction reaction is the reaction between zinc and hydrochloric acid. In this reaction, zinc metal (Zn) is oxidized to zinc ions (Zn2+), while hydrogen ions (H+) in the acid are reduced to hydrogen gas (H2). The balanced equation for this reaction is:
Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g)
In this reaction, zinc loses two electrons (oxidation) and hydrogen gains two electrons (reduction). Therefore, this reaction is classified as an oxidation-reduction reaction.
Another example is the reaction between copper and silver nitrate. In this reaction, copper metal (Cu) is oxidized to copper ions (Cu2+), while silver ions (Ag+) in the silver nitrate are reduced to silver metal (Ag). The balanced equation for this reaction is:
Cu (s) + 2AgNO3 (aq) → Cu(NO3)2 (aq) + 2Ag (s)
In this reaction, copper loses two electrons (oxidation) and silver gains two electrons (reduction). Hence, this reaction is also classified as an oxidation-reduction reaction.
One more example is the reaction between potassium permanganate and sulfuric acid. In this reaction, potassium permanganate (KMnO4) is reduced to manganese dioxide (MnO2), while sulfuric acid (H2SO4) is oxidized to sulfur trioxide (SO3). The balanced equation for this reaction is:
2KMnO4 (aq) + 5H2SO4 (aq) → K2SO4 (aq) + 2MnSO4 (aq) + 5SO3 (g) + 8H2O (l)
In this reaction, potassium permanganate gains five electrons (reduction) and sulfuric acid loses five electrons (oxidation). Therefore, this reaction is classified as an oxidation-reduction reaction.
In conclusion, all the reactions mentioned above involve the transfer of electrons between reactants, making them oxidation-reduction reactions. These examples highlight the importance of oxidation-reduction reactions in various natural and industrial processes.
