Oxidation-reduction reactions are very important in everyday life, as well as in the chemistrylaboratory. Give three examples of oxidation-reduction reactions that might be made use of in everydaylife: describe the reaction, what the reaction is used for and why it is important, and the chemicalreactions involved (if known).2.112© 2015 Cengage Learning. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly accessibie website, an wituile s ingo

The Oxidation-reduction reactions are the type of reactions where oxidation and reduction takes…

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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 4ALQ

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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?
Q6. The reaction of NH3 and O2 forms NO and water. The NO can be used to convert PA to P,06, forming N2 in the process. The P,O can be treated with water to form HyPO3, which forms PH and H3POA when heated. How many grams of NH are needed to produce 20.44 g of PHz? Q9. The purity of a refined silicon sample can be tested by the redox reaction between NaOH and silicon as seen below. If 76.0 g of NaOH yielded 3.52 g of hydrogen gas, calculate percent impurity by mass. Si(g) + NaOH(aq) + H201) - > Na2SiO3(aq) + H2(g) Q10. A chemistry student was assigned to determine the empirical formula of an unknown compound. She first burns 23.58 g of unknown compound in excess oxygen, 52.33 g of CO2, and 23.56 g of H20 was determined. On a second attempt, the nitrogen content of a 3.72 g of the compound was converted to 1.051 g of nitrogen gas. What is the empirical formula of the compound?
Balance the following redox reactions, to their simplest form, by supplying the correct coefficients before each compound for #s 1-15. The unknown coefficients of the compounds should be whole numbers. Note: The reactions below are not yet balanced.
Balance the following redox reaction, which occurs in acidic solution, using the smallest whole-number coefficients: Te(s) + NO3–(aq) → TeO2(s) + NO(g) unbalanced When this equation is appropriately balanced, what is the coefficient on water, and on which side of the equation does water appear? Group of answer choices 6, on the product side 2, on the product side 2, on the reactant side 4, on the reactant side Water does not appear in the balanced equation
Nitric acid, HNO3, can be produced by reacting high-pressure ammonia (NH3) gas with oxygen gas at around 750° C in the presence of a catalyst. Water is a by-product of the reaction. Write the chemical equation for this process. (Ignore balancing) Classify the reaction. Also if this reaction is a redox reaction identify the reduction process and the oxidation process as well as labelling the oxidizing and reducing agents
Specify which of the following are oxidation-reduction reactions, and if it is, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. If it is not, select No and leave the following boxes blank. Express your answers as a chemical formulas. Omit states-of-matter.
(A) if both sentences are true,(B) if both sentences are false,(C) if the first sentence is true but the second is false, and(D) if the first sentence is false but the second is true. 1. In a redox reaction, the oxidation number of iron changed from +2 to +3; thus, sulfur is a reducing agent. In a redox reaction, the oxidation number of nitrogen was unchanged; thus, nitrogen is an oxidant. 2. In a redox reaction, the reducing agent is oxidized and it gains electrons. In a redox reaction, the oxidizing agent is reduced and it gains electrons. 3. Bending stress is also known as flexural stress. The test used in observing the mechanical strength of chocolate is the three-point bend test. 4. The flexural strength of materials may be expressed in Pascals. Magnesium is more reactive than silver; therefore, magnesium corrodes faster than silver with the aid of air, oxygen, and sea water.
Iron corrodes to produce rust, Fe2O3, but other corrosion products that can form are Fe(O)(OH), iron oxyhydroxide, and magnetite, Fe3O4. It turns out that there are two different kinds of Fe in magnetite that have different oxidation numbers. Suggest what these oxidation numbers are and what their relative stoichiometry must be, assuming oxygen's oxidation number is -2 Select all that apply. 1 Fe(IV) 2 Fe(III) 2 Fe(II) 1 Fe(II) 2 Fe(IV) 1 Fe(III)
When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown? F- + Cl2 Cl- + F2Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is reduced? --- When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown? MnO2 + NO2- N2O + MnO4-Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which species is the reducing agent?
Balance the following using the half-reaction method. Identify oxidation, reduction, reducing agent, oxidizing agent. i. Be(NO3)2 (aq) + Ce(s)--> Ce(NO3)3(aq) + Be(s) ii. A container contains H2SO3, H2SO4, Pb2+, Pb4+ and NO3- in distilled water. Create a balanced chemical reaction (Net Ionic Equation, including states of matter) for the spontaneous reaction in the container
The first reaction you will be performing is the reduction of the permanganate ion MnO4– by the iron (II) ion Fe2+ in acidic conditions to standardize the concentration of the perman- ganate solution; the unbalanced chemical equation for the reaction is MnO4– (aq) + Fe2+ (aq) → Mn2+ (aq) + Fe3+ (aq) (d) In the balanced balanced chemical equation for the redox reaction, how many electrons are transferred per mole of permanganate ions? (e) How many moles of iron (II) ions are necessary to completely react one mole of perman- ganate ions?
4.112 A metallurgical firm wishes to dispose of 1300 gallons of waste sulfuric acid whose molarity is 1.37 M. Before disposal, it will be reacted with calcium hydroxide (slaked lime), which costs $0.23 per pound. (a) Write the balanced chemical equation for this process. (b) Determine the cost that the firm will incur from this use of slaked lime.

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