r The cell potential (Ecell) is 1.80 V for a galvanic cell made using the redox couples H+/H₂ and Au³+/Au(s) at 298 K when the concentration of Au(NO3)3 is 0.92 M and the partial pressure of H₂ = 1.3 atm. What is the pH of the anode solution? Au³+ (aq) + 3 e E° = 1.52 V 3.34 0.71 4.69 O 0.55 4.75 O 3.26 → Au(s)

r The cell potential (Ecell) is 1.80 V for a galvanic cell made using the redox couples H+/H₂ and Au³+/Au(s) at 298 K when the concentration of Au(NO3)3 is 0.92 M and the partial pressure of H₂ = 1.3 atm. What is the pH of the anode solution? Au³+ (aq) + 3 e E° = 1.52 V 3.34 0.71 4.69 O 0.55 4.75 O 3.26 → Au(s)

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

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2VO₂ (aq) + 4H* (aq) + Fe (s) → 2VO²+ (aq) + 2H₂O (1)+Fe²+ (aq) Suppose the cell is prepared with 3.37 M VO and 3.31 MH* in one half-cell and 6.13 M VO²+ and 2.52 M Fe²+ in the other. 2+ 2+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28
Suppose a galvanic cell is established using the following cell reaction, Cu(s) + 2Ag+(0.100 M) Cu2+(0.200 M) + 2Ag(s) Each compartment of the cell contains 125 mL of solution. How long would it take at a constant current of 0.10 A for the potential to drop by 10%? By how many grams will the total mass of the two electrodes change during this time period? The change in mass of the copper electrode = g The change in mass of the silver electrode = g The total change in mass of the two electrodes =
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
For the galvanic cell at 298 K 2X(s) + 3Y2*(aq) –→ 2x3*(aq) + 3Y(s) E° cell = 0.39 V What is the measured cell potential (Ecell) when [Y2*] = 1.0 M and [X3+] = 0.01 M? Periodic Table and Datasheet O 0.39 V O 0.35 V O 0.43 V O 0.51 V
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative
Use the Nernst equation to Calculate the cell potential E for the Galvanic cell at 25ºC U=while using the Nernst equation. Al Ι Al3+(aq) ΙΙ Au3+(aq) Ι Au [Al3+(aq)] = 3.00 mol / L , [Au3+(aq)] = 5.00 x 10-5 mol / L. The standard cell potential is E0 = +3.08 V.
The cell potential was 1.271 V at 25oC and a Al3+(aq) concentration of 0.178 M. What was the hydronium ion concentration? The H2(g) pressure was 1 atm at 25oC.6H+(aq) + 2Al(s) ↔ 2Al3+(aq) + 3H2(g) Ecoell = 1.660 V
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =
Use the biological standard potentials of two reduction reactions 4H* + 4e + 02-> 2 H20, E = + 0.82 V NAD* + H* + 2e -> NADH, E = -0.32 V applied to the electrochemical cell NADH|NADH+ ||O2|H20 Write the cell redox reaction and calculate: (a) Thermodynamic standard potentials of two reduction reactions (b) Thermodynamic standard cell potential (c) Thermodynamic standard Gibbs energy of the cell
Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are Fe3+ (aq) + 3 e- → Fe(s) H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1) E' = -0.04 V E' = -0.8698 V K =
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Nit] = 0.00170 M and [Au] = 0.868 M. Standard reduction potentials can be found in this table. %3D 3 Ni(s) + 2 Au*(aq) 3 Ni?+(aq) + 2 Au(s) E = V