101/1 pointYou have a sample of each of the following substances under standard conditions:Ce4+, Ce3+, Fe 2+, Fe 3+, Fe, Mg, Mg2+, Ni 2+, SnSelect all correct answersThe strongest oxidizing agent is Ce4+The strongest reducing agent is Mg2+Fe will dissolve in 1.0 M Ce4+Sn could be oxidized by H+

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Answered: 10 1/1 point You have a sample of each…

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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Use E values to predict which of the following metals, if coated on iron, will provide cathodic protection against corrosion to iron. (a) Cu (b) Mg (c) Ni (d) Sn
Four metals, A, B, C, and D, exhibit the following properties. (i) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (ii) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (iii) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.
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)?
Answer the following questions using data from Table 17-1 (all under standard conditions). a. Is H2(g) capable of reducing Ni2+(aq)? b. Is Fe2+(aq) capable of reducing VO2+(aq)? c. Is Fe2+(aq) capable of reducing Cr3+ (aq) to Cr2+ (aq)?
An equilibrium is established according to the following equation Hg22+(aq)+NO3(aq)+3H+(aq)2Hg2+(aq)+HNO2(aq)+H2O(l)Kc=4.6 What will happen in a solution that is 0.20 M each in Hg22+, NO3-, H+, Hg2+, and HNO2? (a) Hg22+ will be oxidized and NO3- reduced. (b) Hg22+ will be reduced and NO3- oxidized. (c) Hg22+ will be oxidized and HNO2 reduced. (d) Hg22+ will be reduced and HNO2 oxidized. (e) There will be no change because all reactants and products have an activity of 1.
Using Table 17.1, arrange the following reducing agents in order of increasing strength. Br- Zn Co PbSO4 H2S (acidic)
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Which of the following statement(s) is/are true? a. Copper metal can be oxidized by Ag+ (at standard conditions). b. In a galvanic cell the oxidizing agent in the cell reaction is present at the anode. c. In a cell using the half reactions Al3+ + 3e Al and Mg2+ + 2e Mg, aluminum functions as the anode. d. In a concentration cell electrons always flow from the compartment with the lower ion concentration to the compartment with the higher ion concentration. e. In a galvanic cell the negative ions in the salt bridge flow in the same direction as the electrons.
. Assign oxidation sates to all of the atoms in each of the following: a. NH3 b.CO C. CO2 d. NF3
For a voltage-sensitive application, you are working on a battery that must have a working voltage of 0.85 V. The half-cells to be used have a standard cell potential of 0.97 V. What must be done to achieve the correct voltage? What information would you need to look up?
For the following half-reactions, answer these questions. Ce4+(aq)+eCe3+(aq)E=+1.61VAg+(aq)+eAg(s)E=+0.80VHg22+(aq)+2e2Hg(l)E=+0.80VSn2+(aq)+2eSn(s)E=0.14VNi2+(aq)+2eNi(s)E=0.24VAl3+(aq)+3eAl(s)E=1.68V (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce Ag+(aq) to Ag(s)? (f) Will Hg(l) reduce Sn2+(aq) to Sn(s)? (g) Which ion(s) can be reduced by Sn(s)? (h) Which metal(s) can be oxidized by Ag+(aq)?
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.

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