How to choose a reduced or oxidated form in a redox

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SUMMARY

The discussion focuses on determining the correct reduction/oxidation reaction involving copper and chromium in an acidic environment. The participant proposes three unbalanced reactions involving copper (Cu) oxidizing to Cu2+ and reacting with HCrO4-. The consensus indicates that chromium typically reduces to Cr3+ in such reactions, and the correct reaction should reflect this. The importance of understanding oxidation states and common reduction products is emphasized for accurate reaction formulation.

PREREQUISITES
  • Understanding of oxidation and reduction concepts in redox reactions
  • Familiarity with acid-base chemistry, specifically involving sulfuric acid (H2SO4)
  • Knowledge of common oxidation states of transition metals, particularly chromium and copper
  • Ability to write and interpret chemical equations
NEXT STEPS
  • Study the oxidation states of transition metals, focusing on chromium and copper
  • Learn about balancing redox reactions using the half-reaction method
  • Research the solubility rules for metal compounds, particularly copper chromate
  • Explore the role of acids in redox reactions and their effect on oxidation states
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Chemistry students, educators, and anyone interested in mastering redox reactions and understanding the behavior of transition metals in acidic environments.

Peppe
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Hi guys I'm studying about general chemistry in a physics class.
I've some exercices that I'm unable to solve, stuff like this:Copper can be solubilizated in water, oxidating in Cu++ form, reacting with HCrO4- in an acid environment realized by H2SO4. Write down the balanced reaction.my problem is to write (not to balance) an reduction/oxidation reaction.The copper is oxidating, so cromium or hydrogen have to reduce. I've thought about 3 different reaction.
So, in my proposal, the unbalanced reaction are:

Cu + HCrO4- -> Cu++ + Cr2O3 + H2O
Cu + HCrO4- -> Cu++ + CrO + H2O
Cu + HCrO4- -> CuCrO4 + H2

how to choose the correct one?
ciao!
 
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Cr usually gets reduced to Cr3+ in such situations. You are probably right about copper chromate precipitation.

Please note: copper is not "oxidating", copper is "being oxidized" while chromium is being reduced.
 
Thanks for the reply :) :) .

But how can i learn what usually a species does? :O
 

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