Sketch the cell and write the line notation.• 2Ag+ + Cu → Cu2+ + 2AgAg (aq) + eFe3+(aq) + eO2(g) +2 H(aq) + 2eMnO4 (aq) + e2(s) + 2eCu+(aq) + e→Ag(s)0.80Fe2+(aq)0.77→H₂O₂(aq)0.70MnO4(aq)0.56→2(aq)0.54→Cu(s)0.52→→→→4 OH(aq)0.40→ Cu(s)0.3402(g) + 2 H2O(l) + 4 e¯¯Cu2+(aq) + 2eE cell1 = E° SRPcathode - E° SRPanode or E° cell = E° SRPred - E° SRPOX

To sketch the electrochemical cell and write the line notation for the given reaction:2Ag+ + Cu →…

Answered: Sketch the cell and write the line…

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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An electrochemical cell is based on these two half-reactions: Oxidation: Cu(s) → Cu2+(aq, 0.010 M) + 2 e− Reduction: MnO4 −(aq, 2.0 M) + 4 H+(aq, 1.0 M) + 3 e− → MnO2(s) + 2 H2O(l) Calculate the cell potential.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X
Select each of the following electrons that are more likely than that of the standard hydrogen electrode Cu²+ (aq) + 2e → Cu (s) Fe³+ (aq) + e → Fe²+ (aq) Ni²+ (aq) + 2e → Ni (s) F2 (g) + 2e → 2 F¯ (aq) Li+ (aq) + e Li (s)
A chemist designs a galvanic cell that uses these two half-reactions: 3+ 2+ Fe (aq)+e → Fe (aq) Cro (aq) + 4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is half-reaction spontaneous as written. 0 standard reduction potential Ed=+0.771 V 'red E 'red = -0.13 V ロ→ロ × x10 5
Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017
Sketch the cell and write the line notation. • 2Ag++ Cu → Cu2+ + 2Ag Ag (aq) + e Ag(s) 0.80 Fe3+(aq) + e Fe2+(aq) 0.77 O2(g) +2 H(aq) + 2e →H₂O₂(aq) 0.70 MnO4 (aq) + e MnO4(aq) 0.56 2(s) + 2e 21 (aq) 0.54 Cu+(aq) + e Cu(s) 0.52 O2(g) + 2 H2O(l) + 4 e¯ 4 OH(aq) 0.40 Cu2+(aq) + 2e → Cu(s) 0.34 E° cell = E° SRPcathode - E° SRPanode or E° cell = E° SRPred Es SRPOX
Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Cd2+ (aq) + Zn(s)→→→→→→ Cd(s) + Zn²+ (aq) Answer: kJ K for this reaction would be than one.
Balance the following redox equation to its lowest integer ratio. (Under Acidic Conditions) Te(s) + Ru(NO3)3(aq) + NO2(g) ↔ Ru2Te3(s) + HNO3(aq) Note that H2O and H+ are not shown in the equation above. If it is required to balance the equation, then add these.Fill in the coefficient for each chemical after you finish balancing the equation. If the chemical is not needed in the equation then mark a zero next to it Te(s) HNO3(aq) H2O(l) Ru2Te3(s) NO2(g) Ru(NO3)3(aq) H+ (aq)
Using data in the Table, what is the equilibrium constant for the reaction: 2Fe 3+(aq)+H 2(g) 2Fe 2+(aq) + 2H +(aq)?
Calculate the cell potential given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: +0.64 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: +0.44 V
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy following redox reaction. Be sure your answer has the correct number of significant digits. H₂(g) + 2OH¯(aq) + 2Fe³+ (aq) → 2H₂O (1) + 2Fe²+ (aq) kJ x10 X Ś AGO for the
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu²+ (aq) + 2Cu+ (aq) → Cu(s) + 2Cu²+ (aq) 2+ Cu²+ (aq) + 2e → Cu(s) Ee = 0.337 V red 0.153 V = 2+ Cu²+ (aq) +e → Cut (aq) E red AG° kJ K for this reaction would be than one.

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