How do I figure this out? 11. In warm, acidic, aqueous conditions the following reaction can take place (unbalanced, spectator ionsomitted):I0, + V* →I + V5+(a) Which element is oxidized?Which is reduced?(b) Determine the balanced net ionic equation in acidic conditions using thehalf-reaction method.Note: you should showsome evidence of yourthought process inyour response.(c) If 50. mL of a 0.30 M solution of potassium periodate, KIO, (aq) is used for this reaction, how many grams ofV*(aq) will be produced? Assume the reaction only proceeds in the forward direction (as written) and with anexcess of dissolved VCl, (aq).(d) Suppose the cap were left off the container of 0.30 M solution of KIO4 such that some of the waterevaporated. 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 theydon't ask you to. This helps the reader understand your explanation) (e) It turns out that compounds of V* are very unstable in the presence of oxygen gas or oxide ions. Reactionslike these below can occur sequentially, even at room temperature. Comment on changes in vanadium's oxidationstate (if any) in each reaction (oxidized, reduced or no change)4V3+ + 1002- → 2V,O52V,0, → 4VO, +O,2VO, + 4H*→→2VO2* + 2H,OTrivia: 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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11. In warm, acidic, aqueous conditions the following reaction can take place (unbalanced, spectator ions omitted): I0, + V* →F + V$+ (a) Which element is oxidized? Which is reduced? (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 your response. (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 VCI, (aq).

11. In warm, acidic, aqueous conditions the following reaction can take place (unbalanced, spectator ions omitted): I0, + V* →F + V$+ (a) Which element is oxidized? Which is reduced? (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 your response. (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 VCI, (aq).

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter18: Oxidation–reduction Reactions And Electrochemistry

Section: Chapter Questions

Problem 74AP: . To obtain useful electrical energy from an oxidation-reduction process, we must set up the...

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Concept explainers

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

Question

How do I figure this out?

11. In warm, acidic, aqueous conditions the following reaction can take place (unbalanced, spectator ions
omitted):
I0, + V* →I + V5+
(a) Which element is oxidized?
Which is reduced?
(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
your response.
(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).
(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)

(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)
4V3+ + 1002- → 2V,O5
2V,0, → 4VO, +O,
2VO, + 4H*→
→2VO2* + 2H,O
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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