Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Textbook Question
Chapter 17, Problem 87AP
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
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A current of 15.0 A is passed through a solution of CrCl2 for 45 min.(a) How many grams Cr is deposited on the cathode?(b) Calculate the volume of Cl2(g) that is obtained at the anode at 1.00 atm and 273 K.
CATEGORY: Chemistry
Iron corrodes to produce rust, Fe2O3, but other corrosionproducts that can form are Fe(O)(OH), iron oxyhydroxide,and magnetite, Fe3O4. (a) What is the oxidation numberof Fe in iron oxyhydroxide, assuming oxygen’s oxidationnumber is -2? (b) The oxidation number for Fe in magnetitewas controversial for a long time. If we assume thatoxygen’s oxidation number is - 2, and Fe has a uniqueoxidation number, what is the oxidation number for Fein magnetite? (c) It turns out that there are two differentkinds of Fe in magnetite that have different oxidationnumbers. Suggest what these oxidation numbers are andwhat their relative stoichiometry must be, assuming oxygen’soxidation number is -2.
34. A galvanic cell is constructed in which the overall reac-
tion is
Cr,O (aq) + 14 H0 (aq) + 61 (aq) –→
2 Cr" (aq) + 3 12(s) + 21 H,O(()
(a) Calculate AE for this cellI.
(b) At pH 0, with [Cr,O ] = 1.5 M and [I] = 0.40 M,
the cell potential is found to equal 0.87 V. Calculate
the concentration of Cr*(aq) in the cell.
Chapter 17 Solutions
Principles of Modern Chemistry
Ch. 17 - Diagram the following galvanic cell, indicating...Ch. 17 - A galvanic cell is constructed in which a Br2Br+...Ch. 17 - A galvanic cell is constructed in which the...Ch. 17 - Prob. 67PCh. 17 - Galvanized steel consists of steel with a thin...Ch. 17 - the electroplating of a silver spoon, the spoon...Ch. 17 - In some old European churches, the stained-glass...Ch. 17 - Consider a galvanic cell for which the anode...
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- An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forwardHalide 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-.arrow_forwardUse Table 17.1 to predict what reaction, if any, will occur if sulfur is added to acidic aqueous solutions of the following species at standard conditions. (a) MgBr2 (b) Sn(NO3)2(c) Cr(ClO3)2arrow_forward
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