11. In warm, acidic, aqueous conditions the following reaction can take place (unbalanced, spectator ions omitted): I0, + V* – F + Vs+ (a) Which element is oxidized? Which is reduced? I (b) Determine the balanced net ionic equation in acidic conditions using the half-reaction method. Note: you should show some evidence of your thought process in V 3t → V St Lid. 2 reautin. V3t VSt + 2e7 your response. duc. reaction: 104 I 104-I+4 H20 IO+8H+→ I +4420 10, +84*+7€→I+4H,0 t. (c) If 50. mL of a 0.30 M solution of potassium periodate, KIO, (aq) is used for this reaction, how many grams of V*(aq) will be produced? Assume the reaction only proceeds in the forward direction (as written) and with an excess of dissolved VCl, (aq). # of moles of KIOy .30mol So, 10-3L -0 016 mnl

The electrode which has less negative reduction potential will act as a cathode and will undergo…

Answered: 11. In warm, acidic, aqueous conditions the following reaction can take place (unbalanced, spectator ions omitted): I0, + V* – F + Vs+ (a) Which element is…

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How do I finish this problem? I’ve done a,b, and c.

11. In warm, acidic, aqueous conditions the following reaction can take place (unbalanced, spectator ions
omitted):
I0,- + V³+ → F + Vš+
(a) Which element is oxidized?
Which is reduced? I
(b) Determine the balanced net ionic equation in acidic conditions using the
half-reaction method.
Note: you should show
some evidence of your
thought process in
V 3+
Ovid.
Y2 reaurion.
V3t VSt + 2 e/
your response.
educ.
2 reaction: IOy
1041+4 H20
IOu +8H+ -> I +4420
10+8H*+7e→ I'+4H,0
7V3*+2 I Oy +I6H+)7 VSt+ 2 I + 8H20
(c) If 50. mL of a 0.30 M solution of potassium periodate, KIO, (aq) is used for this reaction, how many grams of
V* (aq) will be produced? Assume the reaction only proceeds in the forward direction (as written) and with an
excess of dissolved VCl, (aq).
# of moes of KIO4
.30mol
10.015mol
2 mol I0,7 moj Vst
I mol 104- mol Vt
0.01S mol 104 x0.015 mol Vot =0.0525 mol Vst
Mass produced 0.052s mol x 5/91mol = 2.089
(d) Suppose the cap were left off the container of 0.30 M solution of KIO4 such that some of the water
evaporated. Explain the effect of this procedural mishap on the production of V* ions?
(AP Exam Strategy: In lab error questions, try using hypothetical data to show that you are right, even if they
don't ask you to. This helps the reader understand your explanation)
%3D

(e) It turns out that compounds of V" are very unstable in the presence of oxygen gas or oxide ions. Reactions
like these below can occur sequentially, even at room temperature. Comment on changes in vanadium's oxidation
state (if any) in each reaction (oxidized, reduced or no change)
4V$+ + 1002 → 2V,O5
2V,0, → 4VO, + O,
2VO, + 4H*
2VO2* + 2H,0
Trivia: VO2* = vanadyl ion with charge of 2+.
(f) Are conditions right for that last reaction of part (e) to occur in our container? Why or why not?

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