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H2O2 + ClO2 → ClO2 – +O2 Half reaction and balancing?
You need to put your electrons in the first one:
ClO2 + e- => ClO2-
In the second one, you have done nothing with the hydrogen.
H2O2 => O2 + 2H+ + 2e-
Now you must multiply the first one by 2 to get the same number of electrons on both sides:
2ClO2 + 2e- => 2ClO2-
Now add the equations and eliminate the electrons:
H2O2 + 2ClO2 => 2ClO2- + O2 + 2H+
This is now balanced. The charges are the same on both sides and the number of atoms of each element is the same on both sides.
The oxidising agent is the one which gains electrons and is itself reduced. So, yes, it is the ClO2. The reducing agent is the H2O2. This is itself oxidised because it loses electrons to form H+.
H2O2 + ClO2 ClO2 – +O2 Half reaction and balancing? – ClO2 → ClO2 – H2O2 → O2 If so, is the ClO2 the oxidizing agent? then what's the reducing agent? and how do I balance them? Now add the equations and eliminate the electrons: H2O2 + 2ClO2 => 2ClO2- + O2 + 2H+. This is now balanced. The charges are the same on both sides and the number…equation: Cu(s) + HNO3(aq) Cu(NO 3 )2(aq) + NO(g) + H 2 O(l). Follow these steps. The first eight steps work whether the solution is acidic or basic. 1. Convert the unbalanced redox reaction to the ionic form.The unbalanced chemical equation is as follows: H2 O2 (aq)+ClO4− (aq)⟶O2 (g)+ClO2− (aq) All atoms except H and O are balanced. The oxidation number of Cl changes from 7 to 3. The change in the oxidation number is 4. The oxidation number of O changes from -1 to 0…
How to Balance Redox Equations Answers – StuDocu – Al(s) + HCl(aq) → AlCl3(aq) + H2(g). 49) Write the complete balanced equation for the complete combustion reaction expected to occur. between C3H7OH and O2.Take the above equation and make it basic by balancing the remaining H+ (aq) ions with OH- (aq) ions. This makes them H2O (l). Whatever OH- (aq) is added to one side, it must be added to the other. For example… KClO3. (K+)(ClO3In order to balance H2O2 = O2 + H2O you'll need to watch out for two things. First, be sure to count all of H and O atoms on each side of the chemical Be careful when counting the Oxygen atoms on the product side of the equation. Don't forget the O in H2O! For a complete tutorial on balancing all…
Balance the following redox reactions: H2O2(aq) + ClO4^-(aq)… – Cl2O4 (g)+H2O2 (aq)->ClO2-(aq )+O2 (g)+ H+. BarrettArcher BarrettArcher. Answer : The balanced equation is, Explanation : In the ion electron method, the number of atoms in each half reaction and number of electrons must be balanced.Problem 37 Medium Difficulty. Balance each redox reaction occurring in basic aqueous solution. a. H2O2(aq) + ClO2(aq)-ClO2-(aq) + O2(g) b. Al option A. Let's start with the equation for unbalanced Redox reaction provided to us. We have it's too or do. Balance the following redox equations.BaO2 (s)+2 ClO2 (g)→Ba(ClO2)2 (aq)+O2 (g). This is an oxidation-reduction (redox) reaction Products: Ba(ClO2)2. Names: Barium chlorite.