For the reaction 2HBr(aq) + H2O2 (aq) yields Br2(l) +2H2O(l)...?
You need to obtain a balanced net ionic equation in order to answer this question accurately.
Answer:
The partial reactions of this redox reaction are:
2 Br⁻ → Br₂ + 2 e⁻
H₂O₂ + 2 H⁺ + 2 e⁻→ H₂O
Thus the oxidizing agent is hydrogen peroxide and the reducing agent is the bromide ion.
Edit::
In regular symbols
2 Br[-] ---> Br2 + 2 e[-]
H2O2 + 2 H[+] + 2 e[-] ---> H2O
[+] and [-] denote the charges of the components
2 HBr >> Br2 + 2H+ + 2e- >> oxidation half-reaction
H2O2 + 2H+ + 2e->> 2H2O >> reduction half-reaction
------------------------------...
2HBr (aq)+ H2O2 (aq)>> Br2 (l)+ 2 H2O (l)
the oxidizing agent is O : it goes from -1 to - 2
The reducing agent is Br : it goes from -1 tp 0
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