What are the oxidizing and reducing agents, respectively, for this reaction?
2HCl + H2O2 + MnO2--> O2 + MnCl2 + 2H2O
a) H2O2 ; HCl
b) H2O2 ; MnO2
c) MnO2; HCl
d) MnO2; H2O2
The answer is D. After reading the explanation I understand that Mn's oxidation number went from +4 to +2 therefore became reduced and therefore makes MnO2 an oxidizing agent. O2 in H2O2 went from -1 to 0 therefore is a reducing agent.
My question though, is how do I know which of those compounds I need to find oxidation numbers for in order to find the oxidizing and reducing agents? For example, why wouldn't we look for oxidation states of H or Cl in HCl?
Also, when finding oxidation of O in H2O2, I was able to calculate oxidation state as -1 on the reactant side but I was stuck when I tried to find O oxidation state in the product side because there is O2 and 2H2O both in the products and I wasn't sure if I was supposed to calculate for O2 or H2O
Thank you for your help!
2HCl + H2O2 + MnO2--> O2 + MnCl2 + 2H2O
a) H2O2 ; HCl
b) H2O2 ; MnO2
c) MnO2; HCl
d) MnO2; H2O2
The answer is D. After reading the explanation I understand that Mn's oxidation number went from +4 to +2 therefore became reduced and therefore makes MnO2 an oxidizing agent. O2 in H2O2 went from -1 to 0 therefore is a reducing agent.
My question though, is how do I know which of those compounds I need to find oxidation numbers for in order to find the oxidizing and reducing agents? For example, why wouldn't we look for oxidation states of H or Cl in HCl?
Also, when finding oxidation of O in H2O2, I was able to calculate oxidation state as -1 on the reactant side but I was stuck when I tried to find O oxidation state in the product side because there is O2 and 2H2O both in the products and I wasn't sure if I was supposed to calculate for O2 or H2O
Thank you for your help!