Balance the following oxidation-reduction reaction occurring in
an acidic solution using the half reaction method:
CN1-(aq) + MnO4-(aq) --->
CNO1-(aq) + MnO2(s)
Suppose that you have to balance the following half-reaction in
basic solution.
Cr2O72??(aq) ?
Cr3+?(aq)
What is the coefficient on water of the final balanced half-cell
reaction?
A) 5
B) 6
C) 7
D) 8
balance the following oxidation reduction in an acidic solution
Cl2(g) = Cl– (aq) + OCl–(aq)
(hint: this reaction is a disproportionation, meaning the same
element undergoes both oxidation and reduction. Use Cl2 as the
reactant for each of your half reactions)
Please explain. Thank you!
1) Using the half-reaction method, balance the following
oxidation-reduction reaction which occurs in acidic solution. Be
sure to show each step in balancing both half-reactions and how
electrons in each half reaction are balanced.
Mn2+ (aq) + IO4– (aq) → MnO4– (aq) + IO3– (aq)
2) Would you expect ions such as Cu2+ (light blue solutions) and
Ni2+ (light green solutions) to interfere in the analysis of MnO4–?
Why or why not?
3)Explain quantitatively how your value for the
percent...
balance each of the following oxidation/reduction reactions
utilizing the half reaction method,
H2O2 (aq) + Cl2O7 (aq) → ClO2- (aq) + O2 (g) in basic
solution
The following skeletal oxidation-reduction reaction occurs under
acidic conditions. Write the balanced OXIDATION
half-reaction. Include reactants and products.
Fe3++
H3AsO3---------------------Fe2++
H3AsO4