SUMMARY
The reducing agent in the redox equation Cr2O7 2- + 2OH- --> 2CrO4 2- + H2O is Cr2O7 2-. Upon analyzing the oxidation states, chromium in Cr2O7 2- is reduced from +6 to +6 in CrO4 2-, indicating that it is the species undergoing reduction. The change in oxidation number confirms Cr2O7 2- acts as the reducing agent in this reaction.
PREREQUISITES
- Understanding of oxidation states and how to assign them
- Familiarity with redox reactions and their components
- Knowledge of the dichromate ion (Cr2O7 2-) and chromate ion (CrO4 2-)
- Basic skills in balancing chemical equations
NEXT STEPS
- Study the process of assigning oxidation states in various compounds
- Learn about the role of reducing and oxidizing agents in redox reactions
- Explore the properties and reactions of dichromate and chromate ions
- Practice balancing redox equations using the half-reaction method
USEFUL FOR
Chemistry students, educators, and anyone studying redox reactions and oxidation states in chemical equations.