Study this chemical reaction:
2Fe + 3I2---> 2FeI3
Then, write balanced half-reactions describing the oxidation and
reduction that happen in this reaction.
oxidation:
reduction:
The following skeletal oxidation-reduction reaction occurs under
acidic conditions. Write the balanced OXIDATION
half-reaction. Include reactants and products.
Fe3++
H3AsO3---------------------Fe2++
H3AsO4
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
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
Write a balanced chemical equation describing the oxidation of
chlorine gas by the copper (III) to form the chlorate ion and
copper (II) in an acidic aqueous solution. Use the smallest whole
number coefficients possible.
Also, How many electrons are transferred in the redox
reaction?
Write a balanced chemical equation describing the oxidation
of:
iodine solid by the manganese (III) to form the iodate ion and
manganese (II) in an acidic aqueous solution. Use the smallest
whole number coefficients possible. How many electrons were
transferred in this redox reaction?
chloride ion by solid xenon trioxide to produce the chlorine gas
and xenon gas in an acidic aqueous solution. How many electrons
were transferred?
Write a balanced chemical equation for the following chemical
reactions:
A. Aqueous solutions of potassium iodide and silver (I) nitrate
react to form silver (I) iodide precipitate and aqueous potassium
nitrate.
B. Iron wool is heated with oxygen gas to produce gray iron
(III) oxide.
C. Magnesium metal reacts with nitric acid to yield aqueous
magnesium nitrate and hydrogen gas.
D. Tin (II) chlorate decomposes on heating to give solid tin
(II) chloride and oxygen gas.