A cell consisting of a chromium strip and a lead wire, immersed in 1 M aqueous solutions of Cr(NO3)3 and Pb(NO3)2, respectively, was constructed. It was found that chromium strip depleted and certain solid deposited on the lead wire. Which of the following statement(s) is/are TRUE about the cell? A. Cr3+ was oxidized while Pb2+ was reduced. B. Cr served as the anode while Pb served as the cathode. C. Electrons flow from the lead wire to the chromium strip. D. All of the choices

A cell consisting of a chromium strip and a lead wire, immersed in 1 M aqueous solutions of Cr(NO3)3 and Pb(NO3)2, respectively, was constructed. It was found that chromium strip depleted and certain solid deposited on the lead wire. Which of the following statement(s) is/are TRUE about the cell? A. Cr3+ was oxidized while Pb2+ was reduced. B. Cr served as the anode while Pb served as the cathode. C. Electrons flow from the lead wire to the chromium strip. D. All of the choices

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Question five
2. Balance the following reaction using the ion- electron method. a) MnO4 (aq) + C2O4²- (aq) →> MnO2 (s) + CO2 (9) (in acidic solution) Oxidation half- reaction: Reduction half- reaction: Overall balanced equation:
Calculate the amperage required to deposit 41.7 grams of nickel (AW=58.69) from a solution of NiCl2(aq) in 2.26 hours
Use standard reduction potentials to calculate the equilibrium constant for the reaction:Co2+(aq) + Cu(s) Co(s) + Cu2+(aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.Equilibrium constant: G° for this reaction would be than zero.
The following statements all relate to this redox reaction, which occurs in acidic solution:
Use the standard reduction potentials given below to predict if a reaction will occur when Cr metal is put into a 1 M aqueous 2+ Hg²+ solution. 2+ Hg²+ (aq) + 2e¯ → Hg(1) E red - = 0.855 V Cr³+ (aq) + 3e¯ → Cr(s) Ee -0.740 V red = If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) 2Cr(s) + 3Hg²+ (aq) 2Cr³(aq) + 3Hg(1)
6. Suppose you wish to separate Cd²+ from Zn²+ by electrodeposition of metallic cadmium onto an inert cathode from an aqueous solution containing 0.015 M Cd(NH3)4²+, 0.010 M Zn(NH3)4²+, and 1.00 M uncomplexed NH3. You want to deposit 99.99% of the Cd while not depositing any Zn. What is the allowable range of potentials that you can use? Cd(NH3)4²+ + 2e = Cd(s) + 4 NH3 Zn(NH3)4²+ + 2e → Zn(s) + 4 NH3 E = -0.61 V vs. SHE E° -1.04 V vs. SHE
#73