In each of the following reactions, determine whether or not it is a redox react

Question

In each of the following reactions, determine whether or not it is a redox reaction. If the reaction is a redox reaction then: A.) Ideitify if the reaction is disproportionation, a conproportionation, or neither. B.) Ideitify the oxidazing and reducing agents C.) Balance in acidic medium (if the reaction occurs in aqueous media) using smallest whole number coefficients. D.) Determine the number of moles of electrons transferred between oxidizing and reducing agents. If the reaction is not a redox reaction, balance the reaction by inspection.

1.) Na2O2 + H+ ---> O2 + H2O

Explanation / Answer

1) Na2O2 + H+ ---> O2 + H2O

It is an redox reaction

A) The reaction belongs to type : disproportionation

B) Here, Na2O2 is an reducing agent and H+ is an oxidizing agent

C) Balanced equation : 2Na2O2 + 4H+ ---> O2 + 2H2O

D) moles of electron transfered between oxidizing agent and reducing agent = 1 mole of electron

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