Consider the diagram and reaction below to select the best possible answer for the following questions.Ni (s) + 2Ag (aq) → Ni²¹ (aq) + 2Ag (s)Object "X"Solid nickelSolution containing Ni²+1. Which cell is the cathode?[Select]2. In which direction will the electrons flow?3. What is the name of "Object X"?[Select]4. What is the purpose of "Object X" [Select]Cell A[Select]Cell BSolid silverSolution containing Ag¹+

Given cell diagram is : Reaction is : Ni (s) + 2Ag+ (aq) ----------> Ni2+ (aq) + 2Ag (s) 1.…

Consider the diagram and reaction below to select the best possible answer for the following questions . Ni (s) + 2Ag (aq) → Ni2+ (aq) + 2Ag (s) Object "X" Solid nickel Solution containing Ni²+ Cell A 1. Which cell is the cathode? [Select] 2. In which direction will the electrons flow? [Select] 3. What is the name of "Object X"? [Select] 4. What is the purpose of "Object X" [Select] Cell B Solid silver Solution containing Ag¹+

Consider the diagram and reaction below to select the best possible answer for the following questions . Ni (s) + 2Ag (aq) → Ni2+ (aq) + 2Ag (s) Object "X" Solid nickel Solution containing Ni²+ Cell A 1. Which cell is the cathode? [Select] 2. In which direction will the electrons flow? [Select] 3. What is the name of "Object X"? [Select] 4. What is the purpose of "Object X" [Select] Cell B Solid silver Solution containing Ag¹+

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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A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.
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22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)
5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+ i ii Write the balanced half-reaction for the oxidation that occurs. Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction. iv Write the potential for each half-reaction next to it (the values are in your text) V Calculate the cell potential. vi Calculate AG at 25 °C. vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. ix Write the line notation for the cell.
How many moles of Al3+ would be electrolyzed to Al(s) with the same amount of electricity that produces 16.0 g Cu(s) from a solution of Cu(NO3)2?
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A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.
Which half-reaction occurs at the negative electrode (cathode) if the cell is used for silver plating? A. Ag(s) + e¯ ⇒ Ag*(aq) B. Ag(s) → Ag* (aq) + e C. Ag¹(aq) + e¯ ➜ Ag(s) D. Ag (aq) → Ag(aq) + e O A. Ag(s) OB. Ag(s) + e --> Ag+ (aq) --> Ag+ (aq) + e OC. Ag+ (aq) + e --> Ag(s) O D. Ag+ (aq) --> Ag(aq) + e
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14. In a electrochemical cell, metal D can displace Fe?"(aq) but not Mg"(aq). Identify the metal D. D2* (aq) + 2e → D (s) Reduction Half-Reaction V E° red -1.66 3+ Al (aq) + 3e¯ -→ Al (s) 24+ Са (ag) + 2е -> Са (s) 2+ Cu (aq) + 2e → Cu (s) -2.87 +0.34 2+ -0.44 Fe (aq) + 2e → Fe (s) 2+ -2.37 Mg (aq) + 2e Mg (s) 2+ -0.76 Zn (aq) + 2e → Zn (s) A. Al В. Са С. Си D. Zn