1. Write the balanced oxidation and reduction half reactions for
the reaction of (As_2O_3)^3- and I_2. What ion is oxidized and what
ion is reduced?
2. Assuming that 5 mL of 0.006M arsenite solution is subjected
to coulometric titration using a current of 30 mamps. Calculate the
time that the current should be applied to reach the endpoint of
the titration.
1. Write the balanced oxidation and reduction half reactions for
the reaction of As2O3^(3-) and I2. What ion is oxidized and what
ion is reduced?
2. Assuming that 5 mL of 0.006 M arsenite solution is subjected
to coulometric titration as described in this laboratory using a
current of 30 mamps. Calculate the time that the current should be
applied to reach the endpoint of the titration.
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
Show the balanced oxidation and reduction half – reactions
UNDERLINE THE REDUCING AGENT and BOX THE OXIDIZING AGENT in the
final balanced equation:
NiO2 (s) + Ag (s) ------>
Ni2+ (aq) + Ag+
(aq) (Acidic Solution)
Given the following pairs of
half-reactions, please construct a complete balanced
oxidation-reduction reaction for each pair of two
half-reactions:
a) H2= 2H+ +
2e-
Fe2+= à Fe3+ +
e-
b) 1/4O2(g) + H++ e- == ½ H2OH2 =à 2H++ 2e-
C)
2IO3-+ 12H++ 10e-== I2+ 6H2O 2I-= I2+ 2e-
Separate the following redox reactions into half-reactions, and
label each half-reaction as oxidation or reduction.
Part A
Oxidation half-reaction for 2Li(s)+2H+(aq)→2Li+(aq)+H2(g).
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Part B
Reduction half-reaction for 2Li(s)+2H+(aq)→2Li+(aq)+H2(g).
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Part C
Oxidation half-reaction for 2Ag+(aq)+Be(s)→Be2+(aq)+2Ag(s).
Express your...
The following skeletal oxidation-reduction reaction occurs under
acidic conditions. Write the balanced OXIDATION
half-reaction. Include reactants and products.
Fe3++
H3AsO3---------------------Fe2++
H3AsO4
One of the most useful applications of oxidation-reduction
reactions is the production of electricity. Batteries are
“prepackaged” redox reactions which produce electricity. Consider
the redox reaction of aluminum metal reacting with vinegar (acetic
acid). 2 Al + 6 HC2H3O2 º 2 Al(C2H3O2 )3 + 3 H2 or 2 Al + 6 H+ º 2
Al3+ + 3 H2 A battery works by physically separating the oxidation
and the reduction half reactions.
Why does the cardboard need to be soaked in...
Study this chemical reaction:
2Fe + 3I2---> 2FeI3
Then, write balanced half-reactions describing the oxidation and
reduction that happen in this reaction.
oxidation:
reduction:
For the following redox reaction in a galvanic cell, write the
oxidation half-reaction and the reduction-half reaction, and
calculate the standard cell potential of the reaction. Use Table 1
in the Background as needed. Explain how you identified which
half-reaction is the oxidizer and which is the reducer. Balance the
equation. Show your work. (8pts)
Al(s) +
Ag+1(aq)à
Ag(s) +
Al+3(aq)
Please type your answer out
please