zion 2 Calculate the equilibrium constant for the following reaction at 25°C. yet vered Sn(s) + Pb2*(aq) = Sn2+ (aq) + Pb(s) ked out of The standard cell potential of the corresponding voltaic cell is 0.010 V. Flag question O a. 5.2 Fi O b. 2.2 Oc. 3.2 O d. 4.2 hp

zion 2 Calculate the equilibrium constant for the following reaction at 25°C. yet vered Sn(s) + Pb2*(aq) = Sn2+ (aq) + Pb(s) ked out of The standard cell potential of the corresponding voltaic cell is 0.010 V. Flag question O a. 5.2 Fi O b. 2.2 Oc. 3.2 O d. 4.2 hp

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 galvanic cell based on the following half-reactions: Mn2+ + 2e → Mn e° = -1.18 V Fe²+ + 2e¯ → Fe ɛ° = -0.44 V a. Determine the overall cell reaction and calculate e- (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + + E cell b. Calculate G° and K for the cell reaction at 25°C. AG° kJ K = [Pe**] = c. Calculate Ecell at 25°C when = 0.10 M and = 1.5 x 10-5 M. Ecell =
A voltaic cell consists of a Pb/Pb?+ half-cell and a Cu/Cu2+ half-cell at 25 °C. The initial concentrations of Pb?+ and Cu?+ are 0.0530 mol L1 and 1.60 mol L-', respectively. Part B What is the cell potential when the concentration of Cu+ has fallen to 0.240 mol L? Pb?+ (ag) +2 e → Pb(s) E° = 0.13 V Express your answer using two decimal places. Cu (ag) + 2 e → Cu(s) E = 0.34 V Ecal = 0.489 V Submit Previous Answers Request Answer X Incorrect; Try Again Part C What are the concentrations of Pb?+ and Cu?+ when the cell potential falls to 0.36 V? Express your answers using two significant figures separated by a comma. ? [Pb* ]- [Cu*] = mol L Submit Request Answer
Consider a galvanic cell with the following half-reactions: MnO4 + 8 H* + 5e → Mn?+ + 4 H2O E° = 1.51 V I04- + 2 H+ + 2e¯→ IO3 - + H2O E° = 1.60 V i. What is the reduction half-reaction and oxidation half-reaction. ii. What is the balanced overall reaction. iii. What is the standard cell potential, E°cell.
Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e → Mn ɛ° -1.18 V Cd2+ + 2e –→ Cd e° : -0.40 V = a. Determine the overall cell reaction and calculate cell · (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + + E cel b. Calculate AG° and K for the cell reaction at 25°C. AG° kJ K C. Calculate Ecell at 25°C when Ma*] Ca*+ = 1.2 Mn²+ - 0.10 М and x 10-5 М. Ecell =
What is the numerical value for the standard cell potential for the following reaction? 2Cr 3+ (aq) + 3Cu(s) → 2Cr(s) + 3Cu 2+ (aq) a. 2.52 V b.-1.08 V c. 0.40 V d. 1.08 V e. -0.40 V
H11. Consider the voltaic cell H+ (aq, ?? M) H₂(g, 1 atm)||Cu(s) Cu²+ (aq. 0.1 M). Ecell for this cell at 25 C was +0.360V. What was the pH of the anode solution? A. 0 ABCDE B. C. D. E. 0.89 3.2 7.0 11.7
Cell Potential For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode: Ecell Ered (cathode) - Ed (anode) ▼ Tarnish on copper is the compound CuO. A tarnished copper plate i placed in an aluminum pan of boiling water. When enough salt is added so that the solution conducts electricity, the tarnish disappears. Imagine that the two halves of this redox reaction were separated and connected with a wire and a salt bridge. Part A Calculate the standard cell potential given the following standard reduction potentials: A²+ +3e Cu²+ + 20 Express your answer to two decimal places and include the appropriate units. ▸ View Available Hint(s) Ecell = li Value 4 → Units ? Al; E Cu; E 19 of 42 -1.66 V 0.340 V Review | Constants | Periodic Table
If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode
Consider a voltaic cell with the cell notation shown below. Which of the following statements is INCORRECT? C(s) | V³+ (aq) (1 M), VO²+ (aq) (1 M), H* (aq) (1 M) || Cr₂O7²- (aq) (4 M), Cr³+ (aq) (0.5 M), H* (aq) (1 M) | C(s) Given: VO²+ (aq) + 2 H+ *(aq) + e² = √³+ (aq) + H₂O(1) E° = +0.34 V Cr₂O7²- (aq) + 14 H* (aq) + 6 e¯ 2 Cr³+ (aq) + 7 H₂0 (1) E° = +1.33 V T = 298.15 K; R = 8.3145 J/mol-K; F = 96485 J/V-mol e The maximum work that can be generated by the cell is - 520 kJ. O Six moles of electrons are involved in the redox reaction. The equilibrium constant for the standard electrochemical reaction is e²31. O The cell potential (Ecell) is 1.00 V.
The standard cell potential (E°cell) of the reaction below is -0.55 V. The value of A G° for the reaction is J/mol. 12 (s) + 2Br" (aq) → 21 (aq) + Br2 (1) 0.55 5.5 · 5. 10-6 1.1· 105 0.54 none of the above
Suppose the following reaction happening at 25°C Sn(s) + CuSO4(aq) SNSO4(aq) (reaction in equilibrium) Cu(s) + <----- a) Write the left (Anode) and right (Cathode) reactions. b) Calculate the standard cell potential E°Cell· c) Calculate the equilibrium constant “K" of the reaction using the standard potential data table. TABLE 17.1 Standard Reduction Potentials at 25°C (298 K) for Many Common Half-Reactions Half-Reaction e (V) Half-Reaction e° (V) F + 2e 2F Ag* +e - Ag" Co +e →Cơ H,O, + 2H + 2e 2H,0 Ce +e → Ce* PbO, + 4H + so + 2e PbSO, + 2H,0 MnO, + 4H* + 3e MnO, + 2H,O 2e + 2H + IO, 10, + H,0 MnO, + 8H + Se" → Mn* + 4H,0 Au + 3e -→ Au PbO, + 4H + 2e Pb* + 2H,O Ca, + 2e" → 2CI" Cr0,- + 14H + 6e" → 2Cr“ + 7H,0 O, + 4H + 4e 2H,O MnO, + 4H + 2e Mn + 2H,O 10, + 6H + Se → I, + 3H,0 Br, + 2e 2Br -2H +e VO + H,O 2.87 1.99 O, + 2H,0 + 4c → 40H Cu + 2e Cu Hg,Cl, + 2e -→ 2Hg + 2CI AgCI +e Ag + CI so- + 4H + 2e → H,SO, + H,O Cu* + e - Cu* 2H + 2e H; Fe + 3e Fe Pb* + 2e" -→ Pb Sn Ni* + 2e Ni…
10. What is the standard cell potential of the following electrochemical cell at 25°C: Ni(s) I NiCl2(aq) || Cu(NO3)2 (aq) | Cu(s) a. 0.62 V b. -0.62 V с. 0.60 V d. -0.60 V e. 0.095 V enstant fr ther