a piece of platinum metal, Pt. containing 0.850 M Fe 3+ and 0.010M Fe 2*. In the other cadmium metal, Cd, dips into a 0.500 M solution of Cd 2*. ɛ° = +0.771 V for Fe 3+ + e 2 Fe 2+ ɛ° = -0.403 v for Cd 2+ + 2 e 2 cd i. Write the shorthand notation for the cellI. ii. Calculate the standard cell potential, ɛ°. iii. Calculate the equilibrium constant for the cell reaction Calculate the cell notential E

a piece of platinum metal, Pt. containing 0.850 M Fe 3+ and 0.010M Fe 2. In the other cadmium metal, Cd, dips into a 0.500 M solution of Cd 2. ɛ° = +0.771 V for Fe 3+ + e 2 Fe 2+ ɛ° = -0.403 v for Cd 2+ + 2 e 2 cd i. Write the shorthand notation for the cellI. ii. Calculate the standard cell potential, ɛ°. iii. Calculate the equilibrium constant for the cell reaction Calculate the cell notential E

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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2. Write the cell notation and cell diagram; and identify which is in anode and cathode. a. Ag+(aq) + Mg(s) ----> Ag(s) Mg(s) b. AgcI(s) + Fe(s) -----> Ag(s) + Fe+2(aq) + Cl- (aq) c. Fe(s) + H+(aq) -----> Fe+2(aq) + H2(g,1atm) d. Pb+2(aq) + Cr+2(aq) -----> Pb(s) + Cr+3(aq) e. Au+3(aq) + Fe+2(aq) -----> Au(s) + 4 Cl-(aq) + Fe+3(aq) f. K+(aq) + H2O(I) ----> 02(g) + H+ (aq) + K(s) a. Ag'ia + Mg --> Ag Mg b. AgClos + Fe -----> Aga) + Fe* + Clua) c. Fe + H'ag) > Fela + Hae latm d. Pb" + Cr e. Au f. K'ua + HOn > On + H'aa) + Ko --> Pb + Cru -> Au + 4 Cl n) + Fe" + Fe 2. For the above item #1, a-f; write the cell notation and cell diagram; and identify which is in anode and cathode.
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Which of the following metals should be used to reduce X? Mark all that apply. x2+(aq) + 2e- → X(s); E°: 0.22V a. A*(aq)+ e¯→ A(s); E° = 0.80V b. E2+(aq) + 2e¯ → E(s); E° = 0.34V c. G2+(aq) + 2e¯ → G(s); E° = -0.13V d. j*(aq) + e¯ → J(s); E° = -0.35V
Choose the correct answer. For the cell: Cu | Cu^2+ || Ag+ | Ag. What is the cell potential A. 1.14 V B. -0.46 V C. +0.46 V D. -1.14V
Calculate the equilibrium constant, K, for the following reaction at 25˚C. 2 Fe3+(aq) + Cu(s) → 2 Fe2+(aq) + Cu2+(aq) E° = 0.46 V Give your answer in scientific notation (e.g. 211 is 2.11e2)
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2+ Consider an electrochemical cell made up of Cu Cu²+ and Ag | Agt half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 E £º =0 ロ→ロ V 2+ Calculate the standard emf of a cell that uses the Cu Cu²+ and Ag | Ag* half-cell reaction at 25 °C. Round your answer to 3 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. X ปี x10 Ś X Ś
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?
156. Subject :- Chemistry
Calculate the equilibrium constant for the reaction between Sn metal and Zn2+ solution. Sn + Zn2+ ⇋ Sn2+ + Zn Sn2+ + 2 e− → Sn (s) E° = −0.141 V Zn2+ + 2 e− → Zn (s) E° = −0.762 V Group of answer choices 9.86 × 10^20 3.37 × 10^30 3.18 × 10^−11 1.21 × 10^−21
4. Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Use the table of standard reduction potentials from your textbook to complete the following table. The zinc-copper Daniell cell is given as an example. Cu Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this…