Balance the following redox reactions. Show the complete
balanced reduction half and oxidation half reaction, and label each
accordingly. Give the complete balanced reaction.
A.) CN-1 + MnO4-2 --->
CNO-1 + MnO2
B.) S2O3-2 +
IO2-1 ---> I- +
S4O6-2
. Which of the following are redox
reactions?
I: 2 HF(aq) +
Ca(OH)2(aq) →
CaF2(s) + 2
H2O(l)
II: 2 CH3OH(g) + 3 O2(g)
→ 2 CO2(g) + 4
H2O(l)
III: 2 HNO3(aq) + NO(g)
→ 3 NO2(g) +
H2O(l)
(1) Only
I
(2) Only
II
(3) I and
III
(4) II and
III
(5) I, II, and III
3. Balance the following redox reactions that occur in
acidic solution using the half-reaction method.
a. Cr(s) + NO3-(aq) → Cr3+(aq) + NO(g)
b. CH3OH(aq) + Ce4+(aq) → CO2(aq) +
Ce3+(aq)
c. SO32-(aq) + MnO4-(aq) → SO42-(aq) +
Mn2+(aq)
4. Balance the following redox reactions that occur in
basic solution using the half-reaction method.
a. PO33-(aq) + MnO4-(aq) → PO43-(aq) +
MnO2(s)
b. Mg(s) + OCl-(aq) → Mg(OH)2(s) + Cl-(aq)
c. H2CO(aq) + Ag(NH3)2+(aq) → HCO3-(aq) + Ag(s) +
NH3(aq)
Balance the following redox reactions, in base, using the
half-reaction method. Clearly identify each balanced half-reaction
and the overall balanced equation.
C3H8O2 (a) + Cr2O72– (aq) C3H4O4 (aq) + 2 Cr3+ (aq)
1. a) Show the balanced half reactions and the total balanced
reaction for the following redox reaction in acidic solution.
RuO4 + H2SeO3 → Ru3+ + SeO42-
b) Comment on whether you expect this reaction to be
spontaneous. Show all of your work.b
2 (a) Use the Lattimer diagram for chlorine in basic conditions
to determine the potential for reduction of ClO4- to Cl2 .
(b) Write a balanced equation for this half reaction
Balance each of the following reations using the half reaction
method. Show all work
a. Bi(OH)3(S) + Sn(OH)3-(aq)
---> Sn(OH)62- (aq) + Bi(s) (Basic
solution)
b. BrO3-(aq) + Sb3+(aq) --->
Br
- (aq) + Sb5+ (aq) (acidic solution)
Thank
you for your help!
The question asks me to balance the following redox equation
using the half-reaction method:
6) H2O2 (aq) + IO31-
(aq) --> I1- (aq) + O2 (g) (acidic
solution)