Which of the below electrodes behaves like a resistor and is designed to dissipate any chargeimbalance?O a Non-polarizable electrodeOb Silver electrodeOc Copper electrodeOd. Polarizable electrodeEinthoven lawAO a None of theseO b. A complex in lead III is equal to the sum of the corresponding complexes in leads II and 1.OC A complex in lead I is equal to the sum of the corresponding complexes in leads II and III.Od. A complex in lead II is equal to the sum of the corresponding complexes in leads I and III.

Resistor - Passive, two terminal electrical component that implements electrical resistance as a…

Answered: Which of the below electrodes behaves…

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...

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Salt bridge U A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of different Cu²+ concentrations. The left compartment contains 0.272 M Cu²+, and the right compartment contains 1.25 M Cu²+ . Calculate the cell potential for this reaction at 298 K. volts In this copper concentration cell, the compartment on the left is the + and the compartment on the right is the +
the Relerences to access Important values Il needed lor this Salt bridge A concentration cell similar to the one shown is composed of two Al electrodes and solutions of different AIst concentrations. The left compartment contains 0.523 M AI+ , and the right compartment contains 0.380 M AI3+ . Calculate the cell potential for this reaction at 298 K. volts In this aluminum concentration cell, the reaction would proceed spontaneous v from the left to the right compartment from the right to the left compartment
Calculate the cell potential of the electrolytic cell according to the reaction shown below: Br₂ +2Fe²+ → 2Br¯ +2Fe³+ Given that the standard reduction potentials for Br and Fe³+ are +1.09 V and + 0.77 V respectively. A. -0.32 V B. 0.32 V C. 1.86 V D. -1.86 V
2. In the electrolysis of an aqueous Zn(NO3)2 solution, what reactions occur at the anode and at the cathode, assuming standard conditions? O, + 4H + 4e → 2H;O 6° = 1.23 V 2H,0 + 2e → H2 + 20H E° = -0.83V Zn2 + 2e → Zn ɛ° = -0.76 V NO, + 4H + 3e' → NO + 2H20 E° = 0,96 V ANODE: CATHODE:
How long ill it take to deposit 1.5 g of Ag on a metal when a current of 2A is applied to Ag+ solution? A.) 786 sec B.) 706 sec C.) 670.24 sec D.) 607.42 sec
Calculate the potential for each cell as written at 25 °C. Indicate whether the metal electrode in the half-reaction opposite the standard hydrogen electrode, S.H.E., would be the anode or the cathode if the cell was shorted and electrons were allowed to flow freely. S.H.E. Zn2+(aq, 0.0600 M) Zn(s) E;, = -0.762 V Zn²+/Zn The Zn electrode is the .762 Ecell V cathode. Incorrect anode. Pt(s) V3+(aq, 0.215 M), V²+(aq, 0.00540 M) || S.H.E. = -0.255 V v3+/V2+ The Pt electrode is the .255 Ecell V cathode. Incorrect anode.
3. Consider the following half-cell reactions and associated standard half-cell potentials Ag* + e -> Ag Cu2 + 2e -> Cu Ni2 + 2e -> Ni Cr3 + 3e -> Cr a. Write the overall reaction using the list above that leads to the maximum positive standard potential. b. What is the maximum standard potential?
20). Calculate the cell voltage for the electrochemical cell below. Assume standard conditions. Note: Sulfate is not in any of the solutions. Ni(s) /Ni2* (aq, 1.0 M) //Pb²* (aq, 1.0 M) /Pb(s) a. +0.106 V b. +1.935 V C. +0.124 V d. +0.606 V e. None of the above
Draw the structural formula that is consistent with the of the HNMR spectra shown below
When electrochemical cells are used as chemical probes, equilibrium between the half-cells must be established. O True O False
The electrodes in the following electrochemical cell are connected to a voltmeter as shown. The half-cell on the right contains a standard silver-silver chloride electrode (a silver wire coated with AgCl(s), as in questions 5 and 6). AgCl (s) + e- → Ag(s) + Cl- (1 M) E° = 0.2223 V The half-cell on the left contains a silver electrode immersed in 100.0 mL of 1.00 x 10-3 M AgNO3(aq). A porous plug through which ions can migrate separates the half-cells. What is the voltmeter reading after 10.00 mL of 0.0100 M K2CrO4 has been added to the half-cell on the left and the mixture has been thoroughly stirred? Hint: Ksp of Ag2CrO4 = 1.1 x 10-12
What is the standard emf of the cell with the following overall reaction? Use the provided table for the standard reduction potentials of half-reactions. 2Fe2+ + 2Hg2+2Fe3+ + Hg22+ Express your answer in two decimal places. Table 11.1 Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactions Half-reaction F₂+2e-2F- Ag²+ + e → Ag' Co" te - Cot H₂O₂ + 2H+ + 2e →> Ce+eCe³+ PbO₂ + 4H+ SO4 MnO4 + 4H+ 3e 10₁ + 2H+ 2e MnO4 + 8H + Se Au +3e Au PbO₂ + 4H¹ + 2e → Pb²+ + 2H₂O Cl₂ + 2e → 2CI Cr₂O₂ + 14H+6e2Cr³+ + 7H₂O 2H₂0 +2e → PbSO4 + 2H₂O MnO₂ + 2H₂O 10, + H₂O O₂ + 4H+ 4e → 2H₂O MnO₂ + 4H+ 2e →Mn² + 2H₂O 12+ 3H₂O 10, + 6H + Se Br₂ +2e7 →2Br VO₂ + 2H+ c→ VO²+ + H₂O AuCl +3e7 → Au + 4CI™ NO3 + 4H+ 3e7 CIO₂+eClO₂ 2Hg2+2e7 → Hg₂+ Ag +eAg Hg₂+2e → 2Hg Fe³+ + c →Fe²+ Cu Mn² + 4H₂O → NO + 2H₂O O₂ + 2H+ 2e H₂O₂ MnO4 + MnO2- 12+ 2e21 Cute 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09 1.00 0.99 0.96 0.954 0.91 0.80 0.80 0.77 0.68 0.56 0.54…

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Which of the below electrodes behaves like a resistor and is designed to dissipate any charge imbalance? O a Non-polarizable electrode Ob Silver electrode Oc Copper electrode Od. Polarizable electrode