Concept explainers
Calculate the quantity indicated for each of the following electrolyses
a.
b. the time required to reduce
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General Chemistry: Principles and Modern Applications (11th Edition)
- What is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?arrow_forwardAn 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_forwardThe cell potential of the following cell at 25C is 0.480 V. ZnZn2+(1M)H+(testsolution)H2(1atm)Pt What is the pH of the test solution?arrow_forward
- Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)arrow_forwardA solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of these ions would be reduced first at the cathode during an electrolysis? (b) After the first ion has been completely removed by electrolysis, which is the second ion to be reduced? (c) Which, if any, of these ions cannot be reduced by the electrolysis of the aqueous solution?arrow_forwardAn electrode is prepared by dipping a silver strip into a solution saturated with silver thiocyanate, AgSCN, and containing 0.10 M SCN . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.45 V. What is the solubility product of silver thiocyanate?arrow_forward
- 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.arrow_forwardA galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.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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