QUESTION 11A voltaic cell (same as a galvanic cell) is created from a Cu/Cu<* half-cell (E°red = +0.34 V) and an2+Al/AI3+AI/AIS+half-cell (Ered = -1.66 V). Calculate the value of AG for this cell.O A. -1.16 x 10B. -193000 JC. -764000 JD.-1158000kJE. 193000 J

First calculate the Ecell0 value. Observing the given standard reduction potential values shows…

QUESTION A voltaic cell (same as a galvanic cell) is created from a Cu/Cu2+ half-cell (E°red - +0.34 V) and an Al/AI3+ half-cell (E°red --1.66 V). Calculate the value of AG° for this cell. OA 1.16 x 106J O B. -193000 J O C. -764000 J O D.-1158000 kJ O E. 193000 J

QUESTION A voltaic cell (same as a galvanic cell) is created from a Cu/Cu2+ half-cell (E°red - +0.34 V) and an Al/AI3+ half-cell (E°red --1.66 V). Calculate the value of AG° for this cell. OA 1.16 x 106J O B. -193000 J O C. -764000 J O D.-1158000 kJ O E. 193000 J

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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Question 2 Calculate the cell potential of the following voltaic cell. Zn/Zn²+ (0.001 M)||Cu²+ (0.0001 M) Cu a. +1.22 V O b. +0.98 V O c. +1.04 V d. +1.07 V e. +1.10 V
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Which of the following statements is true concerning the voltaic cell shown below? Voltmeter Kt NO,- Cu+ Zn* NO, So, Zn Cu So, NO, NO, Zn Cut II O a. Zn is the anode having a mass that increases with time. O b. Zn is the cathode having a mass that decreases with time Oc The mass of the Zn electrode neither increases nor decreases with time. O d. Zn is the anode having a mass that decreases with time. O e. Zn is the cathode having a mass that increases with time.
The two redox half reactions represented below are combined to create a galvanic cell. Which statements are true regarding this cell? Select all that apply. 2 H+ (aq) + 2 e= H₂(g) Eº = 0.00 V La³+ (aq) + 3 e La(s) Eº = -2.38 V Three electrons are transferred in the overall, balanced reaction for the cell. La³+ is reduced to La(s) at the cathode. The overall, standard cell potential is 2.38 V. La³+ is produced at the anode. H₂(g) is produced at the cathode. La(s) is the oxidizing agent.
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Determine the reduction/oxidation reactions and the rest of the textbook question
Consider a galvanic cell based in the reaction Fe2+ + Cr,O,→ Fe³+ + Cr³* . Cr,03- + 14H* + 6e¯ →2Cr+ + 7H,0 1.33 Fe+ + e→ Fe?+ 0.77 Balance the reaction. What is the coefficient of Fe3+ in the balanced equation? а. 3 b. 6 с. 4 d. 2 e. none of these
half-cell and a are 0.0530 M MISSED THIS? Read Section 20.6 (Page). A voltaic cell consists of a Pb/Pb²+ Cu/Cu²+ half-cell at 25 °C. The initial concentrations of Pb²+ and Cu²+ 2+ and 1.70 M, respectively. What is the initial cell potential? Express your answer using two significant figures. ►View Available Hint(s) IVE ΑΣΦ Ecell: = Submit Part B 2+ What is the cell potential when the concentration of Cu Express your answer using two significant figures. ► View Available Hint(s) [5] ΑΣΦ Ecell = = Submit Part C ? V has fallen to 0.250 M? ? V What is the concentration of Pb²+ when the cell potential falls to 0.350 V ? Express your answers using three significant figures. ►View Available Hint(s)
A voltaic cell is composed of two half-cells shown below. Determine Q (at 298K) for the reaction when AG- -1,011.6 kJ/mol. Au (aq) + 3e Au(s) +1.50 V Ni2 (aq) + 2e Ni(s) -0.25 V Question 14