What Determines Oxidizing and Reducing Agents in Redox Reactions?

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SUMMARY

This discussion focuses on identifying oxidizing and reducing agents in various redox reactions. The reactions analyzed include P4 + Cl2, Sn2+ + Cu2+, Cu + H+ + NO3-, Br2 + SO2 + H2O, and H2SO4 + 2HBr. Participants concluded that phosphorus (P) acts as the reducing agent and chlorine (Cl) as the oxidizing agent in the first reaction, while tin (Sn) and copper (Cu) serve similar roles in the second. The discussion highlights the importance of balancing charges and compounds in redox equations for accurate identification of agents.

PREREQUISITES
  • Understanding of redox reactions and their components
  • Familiarity with oxidation states and balancing chemical equations
  • Knowledge of common oxidizing and reducing agents
  • Basic chemistry concepts related to electron transfer
NEXT STEPS
  • Study the principles of balancing redox reactions using the half-reaction method
  • Learn about common oxidizing agents such as potassium permanganate and dichromate
  • Explore the role of electron transfer in redox reactions
  • Investigate the applications of redox reactions in electrochemistry
USEFUL FOR

Chemistry students, educators, and professionals in chemical research or education who seek to deepen their understanding of redox reactions and their applications.

yuuri14
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balance the following oxidation reduction reactions. which is the oxidizing agent? reducing agent?
()my answer as balance

a) P4 + Cl2 =(4)PCl5 reducing agent P, o agent Cl
b) Sn2+ + Cu2+ = Sn4+ + Cu+ reducing agent Sn, o agent Cu
c)(2)Cu + H+ +NO3 - = Cu2 + NO2 +H20 " No3, " Cu
D) BR2+ (2)SO2 + H2O = (2)H+ (2)Br- + So4 2- " SO, " Br
e) H2SO4 + 2HBr = SO2 +Br2 + (2) H2O " HBr, " H2SO4
 
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yuuri14 said:
balance the following oxidation reduction reactions. which is the oxidizing agent? reducing agent?
()my answer as balance

a) P4 + Cl2 =(4)PCl5 reducing agent P, o agent Cl
not balanced
b) Sn2+ + Cu2+ = Sn4+ + Cu+ reducing agent Sn, o agent Cu
charges not balanced

I'm not sure how to make out the rest of them. Perhaps you could rewrite them in a more standard form?
 

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