Electrodes Solutions Setup 1 Anode Zinc Zn(NO3)2 1.0 M Cathode Silver AgNO3(aq) 1.0 M % error = Setup 2 Anode Zinc Zn(NO3)2 1.0 M Cathode Silver AgNO3(aq) Concentrations Ecell, V 1.548 1.536 Compare the experimental Ecell values to the theoretical Ecell values by calculating percent error using Eqn 8b-4. experimental value literature value literature value aA(aq) + bB(s) CC(aq) + dD(s) 0.50 M x 100 An electrode potential is a measure of the extent to which the concentrations of the species in a half cell differ from their equilibrium values. Consider the reversible half reaction: Setup 3 Anode Cathode Zinc Silver Zn(NO3)2 AgNO3(aq) 1.0 M (Rxn 8b-4) 0.50 M 1.559 (Eqn 8b-4)

Electrodes Solutions Setup 1 Anode Zinc Zn(NO3)2 1.0 M Cathode Silver AgNO3(aq) 1.0 M % error = Setup 2 Anode Zinc Zn(NO3)2 1.0 M Cathode Silver AgNO3(aq) Concentrations Ecell, V 1.548 1.536 Compare the experimental Ecell values to the theoretical Ecell values by calculating percent error using Eqn 8b-4. experimental value literature value literature value aA(aq) + bB(s) CC(aq) + dD(s) 0.50 M x 100 An electrode potential is a measure of the extent to which the concentrations of the species in a half cell differ from their equilibrium values. Consider the reversible half reaction: Setup 3 Anode Cathode Zinc Silver Zn(NO3)2 AgNO3(aq) 1.0 M (Rxn 8b-4) 0.50 M 1.559 (Eqn 8b-4)

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

Consider the following redox reaction which was conducted under acidic medium to answer this question. x2- M3+ XO M+ + + A 0.122 M Na2X (MM = 78.3) aqueous solution was placed in a buret and titrated against a 1.02 g sample of 75.9% pure MCI3 (MM = 57.5) that had been dissolved in an appropriate amount of acid until the redox indicator changed color. Given this information, how mL of titrant were necessary to completely react with the titrand? Use 3 significant figures to report your answer.
Given the following electrode systems and their electrode potentials, Ca2+(aq) + 2e ➡ Ca(s) E = -2.87V Fe 2+(aq) + 2e ➡ Fe(s) E = -0.44V I2(aq) + 2e ➡ I(aq) E = +0.54V Cr2O72- (aq) + 14H(aq) + 6e ➡ 2Cr3+(aq) + 7H2O E = +1.33V Arrange the following species in order of decreasing as oxidizing strength Write a cell diagram when the calcium and iron half cells are coupled and calculate the emf of the cell.
A concentration cell running at 25°C consists of two Al(s)/Al3+(aq) cells. If the concentration of Al3+ at the anode is 4.12 x 10-8 M and the concentration of Al3+ at the cathode is 1.27 M, what is the value of Ecell? (Two decimal places)
Electrodes Solutions Concentrations Ecell, V Setup 1 Anode Zinc Zn(NO3)2 1.0 M Cathode Silver AgNO3(aq)| Zn(NO3)2 1.0 M 1.0 M Anode Zinc 1.548 Setup 2 Cathode Silver AgNO3(aq) 1.536 0.50 M Setup 3 Anode Zinc Zn(NO3)2 0.50 M 1.559 1. Write the RHR, OHR, and the balanced overall reaction of the voltaic cell Cathode Silver AgNO3(aq) 1.0 M
Part A Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag*(aq) +e –→ Ag(s) What mass of silver would plate onto the cathode if a current of 7.9 A flowed through the cell for 78 min? Express your answer to two significant figures and include the appropriate units. Value Units m = Submit Request Answer
727/variants/1189727/take/10/ 08 MULTIPLE CHOICE Question 12 ☆ □ In a zinc-copper cell, Z | Zn² () Zn || Cu + 2 2 (ag) || Cu + 2 (aq) | Cu(s), which electrode is positive? A Cu+2 B Cu(s) c Zn(s) D Zn +2
Esmeralda the electrochemist sets up an experiment in which she plans to electroplate tin metal onto a 2.0 x 2.0 cm2 electrode surface with a 3.0-A current for 60.0 minutes. Sn2+ + 2 e- → Sn(s) Which of the following experimental changes will result in a thicker film of Sn(s) being deposited? (Check all correct answers.) Group of answer choices increasing the deposition time while keeping all other parameters at their original values increasing the electrode surface area while keeping all other parameters at their original values decreasing the electrode surface area while keeping all other parameters at their original values increasing the current while keeping all other parameters at their original values decreasing the current while keeping all other parameters at their original values decreasing the deposition time while keeping all other parameters at their original values
ELECTROCHEMISTRY: Pt(s) |X*(ag). x2+ (aq) | Y(s) Given the line notation: (aq) || Y3+ where: x2+ + e - x* E° = 0.84 V y3+ + 3 e - Y E° = -1.56 V Pt4+ + 4 e - Pt E° = 1.20 V Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Piease include the negative (-) sign
Boxes 1-2 box 1 answer choices: product side, reactant side, or neither side box 2 answer choices: 3, 2, 6, 5, 8, 0, 1, 4, or 7
line notation Pt(s) | X+(aq), X2+(aq) || Y3+(aq) | Y(s) X2+ + e- X+ Eo = 0.34 V Y3+ + 3 e- Y Eo = -2.2 V Pt4+ + 4 e- Pt Eo = 1.20 V Calculate the EMF.
Given the line notation: Pts) IX* (ag), X2* (aq) I| Y3+ (aq) | Y(s) where: x2+ + e - x+ E° = 0.4 V Y3+ + 3 e → Y E° = -1.84 V P4+ + 4 e → Pt E° = 1.20 V Calculate the EMF.
Handwriting not allow please