When the following equation of a redox reaction in acidic solution is properly balanced, what are the coefficients for Cr20,2-, Fe2+ H*, Cr3+, Fe3+, and H20, respectively? _Cr20,2- + _Fe2+ + H* --> _Cr3+ + Fe3+ + _H20 (A) 1, 3, 14, 2, 3, 7; (B) 1, 6, 14, 2, 6, 7; (C) 2, 10, 14, 2, 10, 7; (D) 2, 12, 28, 4, 12, 14

When the following equation of a redox reaction in acidic solution is properly balanced, what are the coefficients for Cr20,2-, Fe2+ H, Cr3+, Fe3+, and H20, respectively? _Cr20,2- + _Fe2+ + H --> _Cr3+ + Fe3+ + _H20 (A) 1, 3, 14, 2, 3, 7; (B) 1, 6, 14, 2, 6, 7; (C) 2, 10, 14, 2, 10, 7; (D) 2, 12, 28, 4, 12, 14

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 68QAP: Calculate the voltages of the following cells at 25°C and under the following conditions: (a)...

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The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
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-.
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
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 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
For a redox analysis of iron, how do you calculate the % (weight/weight) with a mass of the K2Cr2O7 that was diulted to 250.00ml is 1.488 grams, mass of unknown is 0.2839g, and the vol. titrant given was 24.38 ml?
At 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution within the following cell: Saturated Calomel Electrode | Titration solution | Ag(s) for the cell as writted, what is the voltage after the addition of 10.00 mL of the NaI sooution? The reduction potential for the saturated calomel electrode is E=0.241 V. The standard reduction potential for the reaction: Ag++e- ® Ag(s) E0= 0.79993V. The solubility constant of AgI is Ksp=8.3x10-17 Note: the cell potential could be negative since the condditions are non-standard ones. a)0.169 b)0.354 c)0.235 d)2.360 e)0.441
6) Chromium can be electroplated from aqueous potassium dichromate, with thereduction shown below. If a current of 6.0A and a voltage of 4.5V are used:Cr2O7+(aq) + 14H+(aq) + 12e- -> 2Cr(s)+7H2Oa) How many hours would it take to completely convert215mL of 1.25M K2Cr2O7 to elemental chromium?b) How many kilowatt-hours of electrical energy arerequired to plate 1.00 g of chromium?
3. A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.
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.