Consider a galvanic cell based on the following theoretical half-reactions: Half-reaction E (V) M+ + 3e M 0.60 N+ + 4e N 0.32 What is the value of AG° and K for this cell at 25°C? (Enter your answer to two significant figures.) AG kJ K = Submit Answer Try Another Version 10 item attempts remaining

Consider a galvanic cell based on the following theoretical half-reactions: Half-reaction E (V) M+ + 3e M 0.60 N+ + 4e N 0.32 What is the value of AG° and K for this cell at 25°C? (Enter your answer to two significant figures.) AG kJ K = Submit Answer Try Another Version 10 item attempts remaining

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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Consider the following half-reactions Cute Cu E = +0.521 V H₂O₂ +2e H₂O Question 2 - E = +1.776 V Which of the following is the correct balanced chemical equation for a spontaneous redox reaction from the half-cell reactions above. O H₂O₂(aq) + 2 Cu(s) + 2H,O* (og) 2 Cu" (ag) + 2H₂O(1) OH,O, (aq) + 2 Cu(s) 2 Cu (aq) + 4H₂O(l) - Question 3 O H₂O₂(aq) +2 Cu(s) + 2H₂0 (aq) - 2 Cu" (aq) + 4H₂O(!) O H₂O₂(aq) + Cu(s) + 2H,O* (ag) Cu* (og) + 4H₂O(l) What is the potential (V) of the spontaneous, balanced redox reaction?
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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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Score on last try: 0 of 2 pts. See Details for more. You can retry this question below Determine the equilibrium constant, K, for the voltaic cell composed of the following 2 half reactions at 298 K. Sn²+ (aq) + 2e Mn²+ (aq) + 2e Report your answer in the format 2.4E-3. 1.87E-36 Sn(s) Ecell = -0.136 V Mn(s) E= -1.19 V cell Hint: Decide which half-reaction is the reduction reaction and which one is the oxidation reaction by looking at Eº; the oxidation reaction should be reversed, and Er will have the opposite sign. ox 4.0560949048976E+35
A voltaic cell has one half-cell with a Cu bar in a 1.00 M Cu2+ salt and the other half-cell with a Cd bar in the same volume of a 1.00 M Cd2+ salt. Find Ecell, ΔG, and [Cu2+] at equilibrium. Ecell = ___ V ΔG = ___ J [Cu2+] = ___ x 10 ___ M
b. A cell constructed with a Fe|Fe2+ half-cell and a Pb|Pb2+ half cell 1. Determine E°cell (V) NG Info NG 1 2. Write the net ionic equation for the cell. Info Vork Problem 3. Identify the half-cell at the cathode (enter a number 1- 4) 1. Fe2+, (aq) + 2 e → Fe°(s) 2. Fe°(s) → Fe2+ 3. РЬ2+ + 2 e NG (aq) + 2 e → Pb°, Info (s) + 2 e (aq) 4. Pb° > Pb²+, (s) (aq)
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A voltaic cell is composed of the following 2 half reactions: Mn²+ (aq) + 2e → > Mn(s) Ecell = -1.185 V Cu+ (aq) + e Cu(s) Eell = 0.521 V Determine the non-standard state Ecell at 298 K when Mn²+ (aq) = 0.158 M and Cu+ (aq) = 0.663 M. → V
5. Calculate the cell emf for the following reaction at 25°C Answer: Ni(s) + 2Cu²+ (0.010 M) → Ni²+ (0.0010 M) + 2Cu† (1.0 M) V (express in two decimal places)
Determine the Ell of a voltaic cell composed of Ni(s) in a 1.00 M solution of Ni2+ and Cd(s) in a 1.00 cell M solution of Cd²+ at 25.00°C. Ni(s)/Ni²+ Cd(s)/Cd2+ Submit Question E = -0.257 V Eº= -0.403 V V MacBook Pro
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