Question

Hi, I need help with the following oxidation problem: H2O2 (aq) + ClO2 (aq) → ClO2− (aq) + O2 (g) (basic medium)

Answer 1

http://www.chemguide.co.uk/inorganic/redox/definitions.html

Answer 2

Not what I was looking for ...

Answer 3

what u want form this equation @helpme12345654321

Answer 4

Here are the steps to a fool-proof approach:
Step 1: Separate in half reactions.
Step 2: In each half reaction, balance all elements except O & H.
Step 3: Balance O by adding H2O.
Step 4: Balance H by adding H+.
Step 5: Balance charges by adding e-.
Step 6: Multiply all coefficients in 1 or both half reactions by an integer to get the number of e- in the two half reactions equal.
Step 7: Add the 2 half reactions together & cancel out any species that appear on both sides of net reaction.
Step 8: Check that charges and atoms are balanced.

So,
H2O2(aq) ---> O2(g) + 2H+ + 2e-
Cl2O7(aq) + 6H+ + 8e- ---> 2ClO2^-(aq) + 3H2O
======================================
4H2O2(aq) + Cl2O7(aq) ---> 2ClO2^-(aq) + 4O2(g) + 2H+ + 3H2O

Since it is in basic solution, add 2 OH^- to both sides, and consolidate the waters:

4H2O2(aq) + Cl2O7(aq) + 2OH^- ---> 2ClO2^-(aq) + 4O2(g) + 5H2O

Hope that helped!