A chemist designs a galvanic cell that uses these two half-reactions:half-reactionstandard reduction potentialN2(9)+4 H,O(1)+4eNH4(аq)+4 ОН (аq)–1.16 Vʼred2+E=+0.153 V+Cu"(aq)+e-Cu"(aq)ʼredAnswer the following questions about this cell.Write a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode. Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughinformation toYescalculate the cellvoltage understandardNoconditions?Ifyou said it waspossible tocalculate the cellvoltage, do so andenter your answerhere. Round youranswer to 3significant digits.

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

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(9)+4 H,O(1)+4e N,H,(aq)+4 OH (aq) =-1.16 V red 2+ Cu"(aq)+e Cu"(aq) E=+0.153 V red Answer the following questions about this cell. Write a balanced O-0 equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that U happens at the anode.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(9)+4 H,O(1)+4e N,H,(aq)+4 OH (aq) =-1.16 V red 2+ Cu"(aq)+e Cu"(aq) E=+0.153 V red Answer the following questions about this cell. Write a balanced O-0 equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that U happens at the anode.

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 is based on the following half-reactions (both written as reductions) at 25 °C: E° = 1.00 V VO₂+ (aq) + 2 H+ (aq) + e¯ ⇒ VO²+ (aq) + H₂O (1) Zn²+ (aq) + 2e → Zn (s) E° = -0.763 V Determine whether E is larger or smaller than Eº for the following case: [VO₂+] = 0.10 M, [H†] = 2.0 × 10˚² M, [VO²+] = 1.5 M, [Zn²+] = 0.45 M What is the change in Gibbs free energy for this reaction at standard state conditions (A,Gº)?
In the following: Al³+ (aq) + 3e → Al(s) E° = -1.66 V Cr³+ (aq) + 3e → Cr(s) E° = -0.74 V What is the standard cell potential for the corresponding galvanic cell? 0.00 V O-0.92 V +2.40 V +0.92 V O-2.40 V
voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction:3 Pb(s) + 2 Co3+(aq) 3 Pb2+(aq) + 2 Co(s)What is the effect on the cell emf of each of the following changes?(a) Water is added to the cathode compartment, diluting the solution. The positive cell emf rises, becoming more positive.The positive cell emf drops closer to zero. The negative cell emf rises closer to zero.The negative cell emf drops, becoming more negative.No change in cell emf occurs. (b) The size of the cobalt electrode is increased. The positive cell emf rises, becoming more positive.The positive cell emf drops closer to zero. The negative cell emf rises closer to zero.The negative cell emf drops, becoming more negative.No change in cell emf occurs. (c) A solution of 1.0 M Pb(NO3)2 is added to the anode compartment. The positive cell emf rises, becoming more positive.The positive cell emf drops closer to zero. The negative cell emf rises closer to…
Consider a galvanic electrochemical cell constructed using Cr/Cr** and Zn/Zn2* at 25 °C. The following half-reactions are provided for each metal: 3+ Cr**(aq) + 3 e → Cr(s) E°red = -0.744 V Zn2*(aq) + 2 e → Zn(s) E°red = -0.763 V What is the cell potential for this cell at 25 °C when [Zn2*] = 0.0323 M and [Cr3] = 0.1736 M?
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn"(aq)+2e Zn(s) E=-0.763 V "red MnO,(s)+4H (aq)+2e¯ - Mn²"(aq)+2H,0m E=+1.23 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that U happens at the cathode. O OP 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 calculate the cell voltage under standard conditions? Yes O No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 3 significant digits.
A galvanic cell is powered by the following redox reaction: + 2+ HNO₂(aq) + H+ (aq) + Cu¹ (aq) → NO(g) + H₂O(1) + Cu²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 E = V 0-0 e X 00
Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e- X(s) E° = -2.27 V Y3+ + 3e- Y(s) E° = -0.26 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode?
A galvanic cell is powered by the following redox reaction: 2+ 2 Zn²+(aq) + N₂H₂(aq) + 4OH¯(aq) → 2 Zn(s) + N₂(g) + 4H₂O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 0 E = V 00 S
A galvanic cell is powered by the following redox reaction: 3 Cl,(g) + 2 Cr(OH),(s) + 10 OH (aq) 2 Cro, (aq) + 8 H,O(1) 6 Cl (aq) + Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = Round your answer to 2 decimal places. Explanation Check ?? étv 6.
A galvanic cell is powered by the following redox reaction: Br,(1) + H,(g) + 2 OH (aq) - 2 Br (aq) + 2 H,O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. O-0 Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = [y Round your answer to 2 decimal places. Explanation Check O 2022 McGraw Hill LLC. All Riahts Reserved. Terms of Use F étv 17
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br₂(1)+2e → 2 Br (aq) N₂(g) + 4H₂O()+4e N₂H₂(aq)+4 OH (aq) standard reduction potential E 'red E = red +1.065 V - 1.16 V