Consider the redox reactionAg*(aq) + Cu(s) → Ag(s) + Cu²+(aq)Calculate the E'cell and state if the reaction isspontaneous or not.Half-ReactionE (V)+1.36+1.33+1.23+0.96+0.80Clg) + 2e 20 (ag)Cr,0, (ag) + 14H" (aq) + 6e 20 "(ag) + 7H,O)MnO,(s) + 4H"(ag) + 2eNO, (ag) + 4H (aq) + 3eAg (ag) +eFe"tag) +eCu*(aq) + 2e = Cu(s)AgCKs) +e Agis) + CI (ag)so (aq) + 4H*(ag) + 2e S0,(g) + 2H;O()Cu*(ag) +eSn" (ag) + 2e Sn"(aq)2H (ag) + 2ePhMn" (ag) + 2H,O4)NO(g) + 2H,O)Agis)+0.77+0.34+0.22+0.20Ca*(ag)+0.15+0.13Hg)Phis)0.00+ 20-0.13(ag)Sn" (ag) + 2e Sn(s)Ni*(ag) + 20 Ni(s)PHSO8) + H"(ag) + 2e Pb(3) + HSO, (ag)Ca"(ag) + 20Fe"(ag) + 20C"(ag) + 3eZa*(ag) + 2e-0.14-0.25-0.31-0.40Cds)Fe(s)Cris)-0.44-0.74Zna)-0.76-0.46 V and nonspontaneousO +0.46 V and nonspontaneous-0.46 V and spontaneousO +0.46 V and spontaneous

Given reaction: Ag+(aq) + Cu(s) ----->> Ag(s) + Cu2+(aq) Gibbs free energy: Gibbs free energy…

Consider the redox reaction Ag*(aq) + Cu(s) ► Ag(s) + Cu²*(aq) Calculate the E'cell and state if the reaction is spontaneous or not. Half-Reaction E' (V) Clg) + 2e 20 (ag) Cr,0, (ag) + 14H" (aq) + 6e 20 "(ag) + 7H,O) MnO,(s) + 4H"(ag) + 2e Mn"(ag) + 2H,O) NO, (ag) + 4H (aq) + 3e NO(g) + 2H,0(I) Ag (ag) +e Fe"tag) +e Cu*(aq) + 2e = Cu(s) AgCis) +e Agis) + CI (ag) so, (aq) + 4H*(aq) + 2e SO,(g) + 2H,O() Cu?t(ag) +e= Cu"(ag) Sn" (ag) + 2e 2H (ag) + 2e Ph*(ag) + 2e Pb(s) +1.36 +1.33 +1.23 +0.96 Agis) Fe"(ag) +0.80 +0.77 +0.34 +0.22 +0.20 +0.15 +0.13 Sa*(ag) Hg) 0.00 -0.13 2e Sns 2e Ni(s) -0.14 N" (ag) PHSO,s) + H"(ag) + 2e Ph(s) + HSO, (ag) Ca"(ag) + 2e Fe"(ag) + 2e Fe(s) Cr*(ag) + 3e Cris) Za**(ag) + 2e = Zn(s) -0.25 -0.31 Cds) -0.40 -0.44 -0.74 -0.76 O -0.46 V and nonspontaneous O +0.46 V and nonspontaneous O -0.46 V and spontaneous O +0.46 V and spontaneous

Consider the redox reaction Ag(aq) + Cu(s) ► Ag(s) + Cu²(aq) Calculate the E'cell and state if the reaction is spontaneous or not. Half-Reaction E' (V) Clg) + 2e 20 (ag) Cr,0, (ag) + 14H" (aq) + 6e 20 "(ag) + 7H,O) MnO,(s) + 4H"(ag) + 2e Mn"(ag) + 2H,O) NO, (ag) + 4H (aq) + 3e NO(g) + 2H,0(I) Ag (ag) +e Fe"tag) +e Cu(aq) + 2e = Cu(s) AgCis) +e Agis) + CI (ag) so, (aq) + 4H(aq) + 2e SO,(g) + 2H,O() Cu?t(ag) +e= Cu"(ag) Sn" (ag) + 2e 2H (ag) + 2e Ph(ag) + 2e Pb(s) +1.36 +1.33 +1.23 +0.96 Agis) Fe"(ag) +0.80 +0.77 +0.34 +0.22 +0.20 +0.15 +0.13 Sa(ag) Hg) 0.00 -0.13 2e Sns 2e Ni(s) -0.14 N" (ag) PHSO,s) + H"(ag) + 2e Ph(s) + HSO, (ag) Ca"(ag) + 2e Fe"(ag) + 2e Fe(s) Cr*(ag) + 3e Cris) Za**(ag) + 2e = Zn(s) -0.25 -0.31 Cds) -0.40 -0.44 -0.74 -0.76 O -0.46 V and nonspontaneous O +0.46 V and nonspontaneous O -0.46 V and spontaneous O +0.46 V and spontaneous

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

Related questions

Q: When the Cu2+ concentration is 1.16 M, the observed cell potential at 298K for an electrochemical…

A: In the given cell, copper is undergoing reduction at anode and aluminium is getting oxidized at…

Q: 2) Consider the cell notation of the electrochemical cell shown below: graphite(s) | I"(aq) | 12(s)…

A: The electrochemical cell given is,

Q: Write the line notation of the cell. Hint: the compartment that contains VO2+/VO2+ species has an…

A: We have to give line notation of given cell

Q: What is the cell notation for the following redox reaction? Sn2+(aq) + Cu2+(aq)→ Sn4+(aq) + Cu(s)…

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd2+ + 2 e Cd (a)…

Q: Vrite a balanced =quation for the alf-reaction that appens at the athode. Vrite a balanced equation…

A: Zn (s) ----> Zn+2(aq) + 2e HNO2(aq) + H+ + e- ----> NO(g) + H2O(l)

Q: Draw a galvanic represented by the following line notation and calculate the standard cell potential…

Q: Manganese dioxide (MnO2) for use in dry cell batteries is made by electrolyzing solutions of Mn2*…

Q: (c) (c) The magnitudes but not the signs of the standard electrode potentials of two metals, X and Y…

A: Given half-cell reactions are X2+ + 2e- →X; E0 = 0.25 V Y2+ + 2e- → Y; E0 = 0.34 V Also given…

Q: A galvanic cell is established to power a torch, as shown.For this cell, the overall equation will…

A: The given cell diagram is : Options are : Overall cell equation for this reaction = ?

Q: Cr³*(aq) + 3 e¯ → Cr(s) E°red = -0.744 V Zn**(aq) + 2 e → Zn(s) E°red = -0.763 V Given that the…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

Q: Shown below is a galvanic cell with anode compartment b containing anode a and cathode compartment d…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: We have to write the half-reactions at the cathode and the anode and then write the overall balanced…

Q: The following reaction occurs in a galvanic cell. What is the shorthand notation of this cell?…

A: It is based on the concept of electrochemical cell Here we are required to write the…

Q: State which of the following substances will have a standard heat of formation equal to zero, and…

A: Standard heat of formation is the energy change while the formation of 1 mole of any substance. It…

Q: Heart pacemakers are often powered by lithium-silver chromate "button" batteries. The overall cell…

A: For the multiple subparts, I can solve only first three questions.

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: (a) The half-cell equations are; To obtain the given cell reaction, the half-cell reactions are…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag+| = 1.0…

A: Since Ag+(aq) has a higher reduction potential, Ag+(aq) will undergo reduction to Ag(s) and act as…

Q: Consider the diagram of a galvanic cell, which consists of Cu(s)/Cu2+(aq) and Al(s)/Al3+(aq)…

A: The objective of the question is to calculate the standard emf (electromotive force) for a galvanic…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: In the galvanic cell , two half Reaction occur . One at anode and one at cathode . When both the…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Mno, (s) +…

A: The given redox reaction is, MnO2(s)+4H+(aq)+2Cr2+(aq)→Mn2+(aq)+2H2O(l)+2Cr3+(aq) The overall…

Q: half-reaction standard reduction potential MnO,(aq)+2H,0(1)+3e MnO,(s)+4 OH (aq) E=+0.59 V red 2+…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Which chemical reaction is described by the standard cell notation shown below?…

A: The standard cell notation given for the chemical reaction is- Zns/Zn2+aq//Ag+aq/Ags According to…

Q: A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at…

A: Cell delivers = 0.31 A or 0.31 C/sec In 1 sec charges delivered = 0.31 C 32.1 hr = 3600 sec × 32.1…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: First we would write reduction and oxidation half reactions and use given standard reduction…

Q: This is an example of a disproportionation reaction:…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Consider the redox reaction
Ag*(aq) + Cu(s) → Ag(s) + Cu²+(aq)
Calculate the E'cell and state if the reaction is
spontaneous or not.
Half-Reaction
E (V)
+1.36
+1.33
+1.23
+0.96
+0.80
Clg) + 2e 20 (ag)
Cr,0, (ag) + 14H" (aq) + 6e 20 "(ag) + 7H,O)
MnO,(s) + 4H"(ag) + 2e
NO, (ag) + 4H (aq) + 3e
Ag (ag) +e
Fe"tag) +e
Cu*(aq) + 2e = Cu(s)
AgCKs) +e Agis) + CI (ag)
so (aq) + 4H*(ag) + 2e S0,(g) + 2H;O()
Cu*(ag) +e
Sn" (ag) + 2e Sn"(aq)
2H (ag) + 2e
Ph
Mn" (ag) + 2H,O4)
NO(g) + 2H,O)
Agis)
+0.77
+0.34
+0.22
+0.20
Ca*(ag)
+0.15
+0.13
Hg)
Phis)
0.00
+ 20
-0.13
(ag)
Sn" (ag) + 2e Sn(s)
Ni*(ag) + 20 Ni(s)
PHSO8) + H"(ag) + 2e Pb(3) + HSO, (ag)
Ca"(ag) + 20
Fe"(ag) + 20
C"(ag) + 3e
Za*(ag) + 2e
-0.14
-0.25
-0.31
-0.40
Cds)
Fe(s)
Cris)
-0.44
-0.74
Zna)
-0.76
-0.46 V and nonspontaneous
O +0.46 V and nonspontaneous
-0.46 V and spontaneous
O +0.46 V and spontaneous

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1 Electrochemistry

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the following half-reactions: Half-reaction E° (V) Ag*(aq) + e" Co2*(aq) + 2e → Ag(s) 0.799V → Co(s) |-0.280V Zn2*(aq) + 2e → Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Zn2*(aq) oxidize Ag(s) to Ag"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. e 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 spontaneous as written. Do you have enough information to Yes calculate the cell voltage under standard No conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer||V here. Round your answer to 3 significant digits.
A chemist designs a galvanic cell from the following two half-reactions Ered = +0.96 V NO3(aq) + 4H+ (aq) + 3e¯ → NO(g) + 2H₂O (1) Ered +0.153 V Cu²+ (aq) + e¯ → Cut (aq) The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] = V.
Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
(19) Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu²+ (aq) → Cr³+ (aq) + Cut (aq) If the cell is operating at 25°C, what is the value of the equilibrium constant (Keq)? (A) 1.41 x 10¹1 1.19 x 1018 5.53 x 105 2.79 x 1033 1.81 x 10-6 (B) (C) (D) (E)
5. A more complex example where other atoms are involved. Balance the following reaction in basic solution. r (aq) + MnO4 (aq) MnO, (s)+ BrO;" (aq) TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction E'(V) F + 20 H,0,(aq) + 2 H(aq)+2 e 2F(aq) 2.87 Stronger oxidizing agent Weaker 2 H,0 - PBSO (s) +2 H,0) -Mn0(s)+ 2 H,0) Mn (aq) 4 H,O) - Auts) 1.78 reducing agent PO,(s) + 4 H"(ag) + S0,2-(aq) + 2 e 1.69 Mno, (aq)+ 4 H'(aq) 3 e Mno, (aa) + 8 H (aq)+5 e Au (aq)+3e PbO,(s)+ 4 H(aa) + 2 e Cl,(g) + 2 e" 1.68 1.51 1.50 1.46 - P (ag) + 2 HO - 2a(aq) 1.36 1.33 Cr0, (aq) + 14 H'(ag) + 6 e 0+ 4 H (aq) + 4 e MnO(s)+4 H'(aq) +2 e 10, (aq) 6 H'(aq) + 5e Br+2e vo, (aq) + 2 H'(aq) + e NO, (aq) + 4 H°(aq) + 3e CIO+e 2 C"(aq) + 7 H,On - 2 H,O1) 1.23 Mn (aq) + 2 HyOV) 121 ulae) + 3 H,0() 2 Br (ag) - vo"(aq) +H,00 - NO + 2 H,O0 - CIO, (aa) - Agis) 1.20 1.09 1.00 0.96 0.95 Ag"(aa) + e 0.80 Fe (aq) + O+2 H'(aq)+2e - Fe*(aq) 0.77 - H,O,(ag) 0.70 Mn0, Taa) + e Mn0 (aa) 0.56 8) + 2 e…
Balance the REDOX reaction associated with the cell shown below, in acidic medium: 2+ Fe(s) | Fe² || MnO (aq) Mn²) | Pt(s) Μη '(aq) 4(aq)' Enter the number for the coefficient of H₂O in the balanced equation:
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2* (ag) +2A1 (s) –- 3Cu (s) + 2AI³* (aq) 2+ in one half-cell and 4.12 M Al" in the other. 3+ Suppose the cell is prepared with 3.11 M Cu Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.