(a)
Interpretation:
The given
Concept Introduction:
The
(a)
Answer to Problem 16QRT
The
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The carbon atoms in the given redox reaction are balanced. The oxygen atoms are balanced by putting
The above balanced reaction is multiplied by
Thus, the balanced chemical reaction is shown below.
The oxidation number of carbon atom in
The oxidation number of oxygen atom in
(b)
Interpretation:
The given redox reaction is to be balanced and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(b)
Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The hydrogen atoms and chlorine atoms are balanced by putting
The above balanced reaction is multiplied by
Thus, the balanced chemical reaction is shown below.
The oxidation number of hydrogen atom in
The oxidation number of chlorine atom in
(c)
Interpretation:
The given redox reaction is to be balanced in acidic medium and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(c)
Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of titanium atom in
The oxidation number of oxygen atom in
The given unbalanced redox reaction is shown below.
The oxidation number of titanium atom in
The oxidation number of oxygen atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The given reaction is to be balanced in acidic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, now hydrogen atoms are balanced by adding protons
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Since, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
(d)
Interpretation:
The given redox reaction is to be balanced in acidic medium and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(d)
Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of chlorine atom in
The oxidation number of manganese atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The given reaction is to be balanced in acidic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, now hydrogen atoms are balanced by adding protons
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Since the electron gain is not equivalent to electron lost. Thus, multiply the oxidation half reaction by
Oxidation:
Reduction:
Now, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
(e)
Interpretation:
The given redox reaction is to be balanced and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(e)
Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of iron atom in
The oxidation number of oxygen atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The iron atom and sulphur atoms are balanced by putting
Oxidation:
Reduction:
The given reaction is to be balanced in acidic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, now hydrogen atoms are balanced by adding protons
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Since the electron gain is not equivalent to electron lost. Thus, multiply the oxidation half reaction by
Oxidation:
Reduction:
Now, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
(f)
Interpretation:
The given redox reaction is to be balanced and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(f)
Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given redox reaction is shown below.
The given redox reaction is already balanced and there are equal numbers of each atom both the sides.
The oxidation number of nitrogen atom in
The oxidation number of oxygen atom in
(g)
Interpretation:
The given redox reaction is to be balanced in basic medium and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(g)
Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of zinc atom in
The oxidation number of mercury atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The given reaction is to be balanced in basic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, hydrogen atoms are balanced by adding water molecules
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Now, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
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Chapter 17 Solutions
Chemistry: The Molecular Science
- Gold can be dissolved from gold-bearing rock by treating the rock with sodium cyanide in the presence of oxygen. 4 Au(s) + 8 NaCN(aq) + O2(g) + 2 H2O() 4 NaAu(CN)2(aq) + 4 NaOH(aq) (a) Name the oxidizing and reducing agents in this reaction. What has been oxidized, and what has been reduced? (b) If you have exactly one metric ton (1 metric ton = 1000 kg) of gold-bearing rock, what volume of 0.075 M NaCN, in liters, do you need to extract the gold if the rock is 0.019% gold?arrow_forwardXenon trioxide, XeO3, reacts with aqueous base to form the xenate anion, HXeO4. This ion reacts further with OH to form the perxenate anion, XeO64, in the following reaction: 2HXeO4(aq)+2OH(aq)XeO64(aq)+Xe(g)+O2(g)+2H2O(l) Identify the elements that are oxidized and reduced in this reaction. You will note that the equation is balanced with respect to the number of atoms on either side. Verify that the redox part of this equation is also balanced, that is, that the extents of oxidation and reduction are also equal.arrow_forwardThe blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with an acidic potassium di-chromate solution, resulting in the production of Cr3+ (aq) and carbon dioxide. The reaction can be monitored because the dichromate ion (Cr2O72) is orange in solution, and the Cr3+ ion is green. The balanced equations is 16H+(aq) + 2Cr2O72(aq) + C2H5OH(aq) 4Cr4+(aq) + 2CO2(g) + 11H2O(l) This reaction is an oxidationreduction reaction. What species is reduced, and what species is oxidized? How many electrons are transferred in the balanced equation above?arrow_forward
- The Ostwald process for the commercial production of nitric acid involves the Following three steps: 4NH3(g)+5O2(g)4NO(g)+6H2O(s)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) a. Which reaction in the Ostwald process are oxidation-reduction reactions? b. Identify each oxidizing agent and reducing agent.arrow_forwardTriiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: IO3(aq) + I(aq) I3(aq) Triiodide ion concentration is determined by titration with a sodium thiosulfate (Na2S2O3) solution. The products are iodide ion and tetrathionate ion (S4O6). a. Balance the equation for the reaction of IO3 with I ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HQ required to convert all of the IO3 ions to I ions? c. Write and balance the equation for the reaction of S2O32 with I3 in acidic solution. d. A 25.00-mL sample of a 0.0100 M solution of KIO. is reacted with an excess of KI. It requires 32.04 mL of Na2S2O3 solution to titrate the I3 ions present. What is the molarity of the Na2S2O3 solution? e. How would you prepare 500.0 mL of the KIO3 solution in part d using solid KIO3?arrow_forwardOne of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?arrow_forward
- Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus (P4) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4-) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.arrow_forwardDetermine the oxidation states of the elements in the following compounds: (a) Nal (b) GdCl3 (c) LiNO3 (d) H2Se (e) Mg2Si (f) RbO2, rubidium superoxide (g) HFarrow_forwardFour metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.arrow_forward
- The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?arrow_forwardChromium has been investigated as a coating for steel cans. The thickness of the chromium film is determined by dissolving a sample of a can in acid and oxidizing the resulting Cr3+ to Cr2O72 with the peroxydisulfate ion: S2O82(aq) + Cr3+(aq) + H2O(l) Cr2O72(aq) + SO42(aq) + H+(aq) (Unbalanced) After removal of unreacted S2O82 an excess of ferrous ammonium sulfate [Fe(NH4)2(SO4)26H2O] is added, reacting with Cr2O72 produced from the first reaction. The unreacted Fe2+ from the excess ferrous ammonium sulfate is titrated with a separate K2Cr2O7 solution. The reaction is: H+(aq) + Fe2+(aq) + Cr2O72(aq) Fe3+(aq) + Cr3+(aq) + H2O(l) (Unbalanced) a. Write balanced chemical equations for the two reactions. b. In one analysis, a 40.0-cm2 sample of a chromium-plated can was treated according to this procedure. After dissolution and removal of excess S2O82, 3.000 g of Fe(NH4)2(SO4)26H2O was added. It took 8.58 mL of 0.0520 M K2Cr2O7 solution to completely react with the excess Fe2+. Calculate the thickness of the chromium film on the can. (The density of chromium is 7.19 g/cm3)arrow_forwardThe Toliens test for the presence of reducing sugars (say, in a urine sample) involves treating the sample with silver ions in aqueous ammonia. The result is the formation of a silver mirror within the reaction vessel if a reducing sugar is present. Using glucose, C6H12O6, to illustrate this test, the oxidation-reduction reaction occurring is C6H12O6 (aq) + 2 Ag+(aq) + 2OH(aq) C6H12O7(aq) + 2 Ag(s) + H2O() What has been oxidized, and what has been reduced? What is the oxidizing agent, and what is the reducing agent? Tolien's test. The reaction of silver ions with a sugar such as glucose produces metallic silver. (a) The set-up for the reaction. (b) The silvered test tubearrow_forward
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