Identifying redox reactions under cidic and basic conditions
Cr2O7^2-(aq) + NH4^+(aq) == Cr2O3(s) + N2(g)
Please help me to balance this equation in acidic and basic conditions.
How to find the oxidation numbers for EU(NO2)3 .
Please explain Thank you so much.
Cr2O72-(aq) + NH4+(aq) ---> Cr2O3(s) + N2(g)
a) In acidic medium
Oxidation half reaction-- 2NH4+ → NO2 + 6e - + 8H+
Reduction half reaction-- Cr2O72- + 6e- + 8H+ → Cr2O3 + 4H2O
Now, add the half reactions together, we will get,
2NH4+ + Cr2O72- + 6e- + 8H+ → NO2 + Cr2O3 + 6e- + 4H2O + 8H+
=> 2NH4+ + Cr2O72- → N2 + Cr2O3 + 4H2O
b) In basic medium
Oxidation half reaction--- 2NH4+ + 8OH- → NO2 + 6e- + 8H2O
Reduction half reaction-- Cr2O72- + 6e- + 4H2O → Cr2O3 + 8OH-
Now, add both the half reactions together---
2NH4+ + Cr2O72- + 8OH- + 6e- + 4H2O → NO2 + Cr2O3 + 6e- + 8OH- + 8H2O
=> 2NH4+ + Cr2O72- → N2 + Cr2O3 + 4H2O
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