17. (5 pts.) Given the following balanced net ionic equation: Mn + Cr+2 (aq) → Mn*2 (aq) + Cr (s) (s) Answer the following: to include poe A.) (1.5 pts.)Write the oxidation half reaction. Teel thee to B.) (1.5 pts.) Write the reduction half reaction. C.) (0.5 pt.) Which species is being oxidized (be specific)? D.) (0.5 pt.) Which species is being reduced (be specific)? E.) (0.5 pt.) Which species is the oxidizing agent (be specific)?

17. (5 pts.) Given the following balanced net ionic equation: Mn + Cr+2 (aq) → Mn*2 (aq) + Cr (s) (s) Answer the following: to include poe A.) (1.5 pts.)Write the oxidation half reaction. Teel thee to B.) (1.5 pts.) Write the reduction half reaction. C.) (0.5 pt.) Which species is being oxidized (be specific)? D.) (0.5 pt.) Which species is being reduced (be specific)? E.) (0.5 pt.) Which species is the oxidizing agent (be specific)?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 61E: Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the...

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Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
In some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
A 1 M solution of Cu1NO322 is placed in a beaker with astrip of Cu metal. A 1 M solution of SnSO4 is placed in asecond beaker with a strip of Sn metal. A salt bridge connects the two beakers, and wires to a voltmeter link the twometal electrodes. (a) Which electrode serves as the anode,and which as the cathode? (b) Which electrode gainsmass, and which loses mass as the cell reaction proceeds?(c) Write the equation for the overall cell reaction. (d) Whatis the emf generated by the cell under standard conditions?
The iodine produced when excess of KI was added to the solution containing 0.1259 g K2Cr2O7 required a 41.26 mL titration with Na2S2O3 required a 41.26 mL titration with Na2S2O3. P.S. Be able to answer numbers 3 and 4 ONLY. 1. Determine if it is basic or acidic and write the balance redox reaction for the reaction of dichromate ion with iodide ion in acidic medium. Unbalance equation: Cr2O72- (aq) + I- (aq) → Cr3+ + I2 (aq) 2. Determine if it is basic or acidic and write the balance redox reaction of iodine with sodium thiosulfate in acidic medium. Unbalance equation: S2O3 2- (aq) + I2 (aq) → S4O6 2- (aq) + I- (aq) 3. (i) What are the oxidizing agents in #1 and #2? (ii) What is the stoichiometric ratio between dichromate and thiosulfate? 4. Calculate the molar concentration of the thiosulfate solution.
(a) How many coulombs are required to plate a layer ofchromium metal 0.25 mm thick on an auto bumper witha total area of 0.32 m2 from a solution containing CrO42-?The density of chromium metal is 7.20 g/cm3. (b) Whatcurrent flow is required for this electroplating if the bumperis to be plated in 10.0 s? (c) If the external source has anemf of +6.0 V and the electrolytic cell is 65% efficient,how much electrical power is expended to electroplate thebumper?
The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes place in an acidic aqueous solution. The normal reduction potentials of ions Zn2+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).Introducing a Pt electrode in a MnO4-/ Mn2+ solution, with a salt bridge, and putting it together with the other electrodes (Zn, Au or Ag) and their aqueous solutions,a) Comment in which case will the permanganate oxide the metalsb) Justify your answerc) In those cases where the oxidation takes place, write the diagram of the celld) Calculate the standard potential of the cells, Eºcell. Result: a) Eºcell >0 d) 0.7108 V, 0.7482 V
Black-and-white photographic film is coated with silver halides. Because silver is expensive, the manufacturer monitors the Ag⁺ content of the waste stream, [Ag⁺]ᵥᵥₐₛₜₑ, from the plantwith an Ag-selective electrode at 25°C. A stream of known Ag⁺ concentration, [Ag⁺](standard), is passed over the electrode inturn with the waste stream and the data recorded by a computer.(a) Write the equations relating the nonstandard cell potential tothe standard cell potential and [Ag⁺] for each solution.(b) Combine these into a single equation to find [Ag⁺]ᵥᵥₐₛₜₑ.(c) Rewrite the equation from part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ in ng/L.(d) If Eᵥᵥₐₛₜₑ is 0.003 V higher than E(standard), and the standard so-lution contains 1000. ng/L, what is [Ag⁺]ᵥᵥₐₛₜₑ?(e) Rewrite the equation in part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ for a sys-tem in which T changes and Tᵥᵥₐₛₜₑ and T(standard) may be different.
An aqueous solution of NaCl was electrolyzed with a current of 2.50 amps for 15.0 minutes. What volume (in mL) of 0.500 M HCl would be required to neutralize the resulting solution? (Hint: H2 is produced at the cathode and Cl2 at the anode.)
A 15.46 g meat sample is taken, chopped, passed through a blender and the resulting suspension is filtered; obtaining a clean solution containing NO2-. Subsequently, it is treated with 25.00 mL of KMnO4 0.01548 M in acid medium. After 10 min, the remaining KMnO4 is titrated with 14.97 mL of FeSO4 0.08183 M. a) Indicate the redox reactions that take place and adjust them (Note: NO2- oxidizes to NO3- in an acid medium) b) Calculate the NO2- content in mg / kg (MW nitrite, 46.00) Answer: 1056 mg / kg
Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswer
Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswer(ii) Calculate the unknown concentration.(iii) Does your calculated answer agree with your original answer?Why?