Given the following two half reactions write a balanced oxidation-reduction reaction that occurs between sulfite and Ru3+ in acidic solution. Recall that a good way to proceed is to balance each half reaction in acidic solution, adjust one or both to have the same number of electrons gained as lost, and then add them together .. SO32-→ SO42- and Ru3+ → Ru2+ A) H2O + SO3²- + Ru3+ Ru2+ + SO42- + 2H* B) 6 H2O + 2 SO32- + Ru3+ → Ru2+ + 2 SO42- + 12 H* C) H2O + SO3²- + 2 Ru3+ → 2 Ru²+ + SO42- + 2H* A) H2O + SO3²- + 2 Ru3+ → 2 Ru²+ + SO4²- + 2e¯ + 2H*

Given the following two half reactions write a balanced oxidation-reduction reaction that occurs between sulfite and Ru3+ in acidic solution. Recall that a good way to proceed is to balance each half reaction in acidic solution, adjust one or both to have the same number of electrons gained as lost, and then add them together .. SO32-→ SO42- and Ru3+ → Ru2+ A) H2O + SO3²- + Ru3+ Ru2+ + SO42- + 2H* B) 6 H2O + 2 SO32- + Ru3+ → Ru2+ + 2 SO42- + 12 H* C) H2O + SO3²- + 2 Ru3+ → 2 Ru²+ + SO42- + 2H* A) H2O + SO3²- + 2 Ru3+ → 2 Ru²+ + SO4²- + 2e¯ + 2H*

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.28QE

See similar textbooks

Similar questions

Given the following two half reactions write a balanced oxidation-reduction reaction that occurs between sulfite and Ru3+ in acidic solution. Recall that a good way to proceed is to balance each half reaction in acidic solution, adjust one or both to have the same number of electrons gained as lost, and then add them together ...SO32- → SO42- and Ru3+ → Ru2+A) H2O + SO32- + Ru3+ → Ru2+ + SO42- + 2H+B) 6 H2O + 2 SO32- + Ru3+ → Ru2+ + 2 SO42- + 12 H+C) H2O + SO32- + 2 Ru3+ → 2 Ru2+ + SO42- + 2H+D) H2O + SO32- + 2 Ru3+ → 2 Ru2+ + SO42- + 2e- + 2H+
Write the relevant half-reactions, then combine them into a full reaction, for FeS oxidation to Fe2+ and SO42- by O2 going to H2O
Balance the following redox reaction which occurs in acidic solutions: NO2^-1 + Cr2O7^-2 --> Cr^+3 + NO3^-1 1) the balanced reduction half-reaction 2) the balanced oxidation half-reaction 3) The coefficients in order as shown below for all possible reagents and products in the reaction (just list the numbers and a dash between reagents and products.) NO2-1 Cr2O7-2 H2O H+ OH-1 - Cr+3 NO3-1 H2O H+ OH-1
Ozone (O3) and chlorine dioxide (ClO2) are both strong oxidizing agents. Given the half reactions for these species as follow: O3 + 2H+ + 2e- = O2 + H2O, E0 = 2.07 V vs. SHE ClO2 + e- = ClO2-, E0 = 1.15 V vs. SHE Write and balance the overall reaction that occurs when O3 is mixed with NaClO2 in aqueous solution. What is the standard Gibbs free energy for the overall reaction?
(a) Assuming standard conditions, arrange the following in order of increasing strength as oxidizing agents in strong acid:ClO-, ClO3-, O2, IO3-, Mn2+ __ClO- __ClO3- __O2 __IO3- __Mn2+ < __ClO- __ClO3- __O2 __IO3- __Mn2+ < __ClO- __ClO3- __ O2 __IO3- __Mn2+ < __ClO- __ClO3- __O2I __O3- __Mn2+ < __ClO- __ClO3- __O2 __IO3- __Mn2+ (b) Assuming standard conditions, arrange the following in order of increasing strength as reducing agents in strong base:Cl-, Ba, Sn, Na, Bi Cl- Ba Sn Na Bi < Cl- Ba Sn Na Bi < Cl- Ba Sn Na Bi < Cl- Ba Sn Na Bi < Cl- Ba Sn Na Bi
Discuss, in your own words, THREE conditions where corrosion is initiated via electrochemical reactions. (b) A “salt-water drop” experiment was performed on a sheet of clean steel in the laboratory. (i) What is the name of the indicator used? (ii) What did the indicator contain? (iii) Draw a sketch of the results, explaining what colours could be seen and what caused them. (iv) What type of corrosion cell does it demonstrate? The Pourbaix diagram shows the predominant form in which an element will exist under a given set of environmental conditions. Pourbaix diagrams display thermodynamically preferred species. (i) For a given metal what equation is used to construct a Pourbaix diagram? (ii) Three regions are identified in the Pourbaix diagram, what are these regions and what information do they provide? Predict the possibility of galvanic corrosion in sea water for the following coupled pairs of alloys and metals. Using the Galvanic Series Sheet please provide a reason for your…
Match each commercial application of electrochemistry with the appropriate description. a. electroplating b. secondary cell c. cathodic protection d. electrorefining e. fuel cell f. Hall-Heroult process g. dry alkaline battery ____ 1. measures taken to prevent corrosion ____ 2. a battery where the reactants are continuously replenished ____ 3. a primary cell ____ 4. the application of a thin coating of a metal that resists corrosion ____ 5. the use of molten cryolite to produce aluminum ____ 6. a rechargeable battery ____ 7. the process used to obtain high-grade, pure metals from impure materials
1 ANYONE KNOWS?? 4. A standard electrode potential of Pb2+/Pb is measured directly by connecting to a reference electrode in an electrochemical cell. From the observation, bubbles were formed in one of the half-cell. (a) Name the reference electrode used for this purpose. [1] (b) Write the half-cell equations to represent the reaction taking place at: [2] Anode : Cathode :
Write the relevant half-reactions, then combine them into a full reaction for H2AsO3- oxidation to HAsO42- by reducing FeOOH to Fe2+
Make an inference about the effect of applied current and electrolysis time on the mass of deposited copper. Thoroughly explain and relate any observed trend to Faraday’s Law of Electrolysis.a. What happened to the mass of deposited Cu when the applied current is increasedb. What happened to the mass of deposited Cu when the electrolysis time is increased
With regards to observations, what corrosion is happening to each nail being placed in agar plates with iron hexacyanide? (include species that are being oxidised and reduced
A cell consisting of a saturated calomel electrode and a lead ion electrode developed a potential of -0.3257 V when immersed in a 60.00 mL lead solution of unknown concentration. A 10.00 mL addition of 0.02500 M lead standard solution caused the reduction potential to shift to -.2897 V. Calculate the molar concentration (in units mM) of lead in the sample. Please make sure to perform necessary calculations to have a final answer in mM.