In each of the following balanced oxidation-reduction equations,
identify those elements that undergo changes in oxidation number
and indicate the magnitude of the change in each case
Part A
2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq)
Enter your answers as chemical symbols separated by a comma.
Part C
4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g)
Enter your answers as chemical symbols separated by a comma
Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g)
Enter your answers as chemical symbols separated by a comma
In each of the following balanced oxidation-reduction equations,
identify those elements that undergo changes in oxidation number
and indicate the magnitude of the change in each case.
2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq)
4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g)
Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g)
The following skeletal oxidation-reduction reaction occurs under
acidic conditions. Write the balanced OXIDATION
half-reaction. Include reactants and products.
Fe3++
H3AsO3---------------------Fe2++
H3AsO4
Use the rules (in order) to assign oxidation numbers to each of
the elements in the compounds below.
hydroxylamine
H
N
O
NH2OH
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
magnesium bromide
Br
Mg
MgBr2
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
boric acid
H
B
O
H3BO3
determine the balanced thermochemical equation for the oxidation of
one mole of sucrose. is the reaction gaining or losing energy?
(Show this with an equation)
Determine the energy generated by eating one serving of jelly
bellies by calculating based on grams of sucrose per serving of
jelly belly
When the following oxidation–reduction reaction in a basic
solution is balanced, what is the lowest whole-number coefficient
for OH−and on which side of the balanced equation should it
appear?
S2O82–(aq)+NO(g)→SO42–(aq)+NO3–(aq)
a. 4, product side
b. 8, reactant side
c. 12, reactant side
d. 8, product side
e. 4, reactant side
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
When the following oxidation–reduction reaction is balanced with
lowest whole-number coefficients, what is the coefficient for
Mn2+(aq)?
__MnO4–(aq) + __C2H5CHO(aq) + __H+ (aq) → __Mn2+(aq) +
__C2H5COOH(aq) +__ H2O(l)
When I balanced this equation I got the following:
1MnO4–(aq) + 1C2H5CHO(aq) + 6H+ (aq) → 1Mn2+(aq) + 1C2H5COOH(aq)
+3 H2O(l)
so therefore, the answer would be 1. However, the answer is 2.
Can someone explain why the answer is 2 and what I did wrong?