A chemist designs a galvanic cell that uses these two half-reactions:half-reactionstandard reduction potential2+Cu"(aq)+eCu (aq)E=+0.153 v2 I0, (aq)+12 H (aq)+10eL(s)+6 H,O(1)E=+1.195 VredAnswer the following questions about this cell.Write a balancedequation for thehalf-reaction thathappens at thecathode.eWrite a balancedequation for thehalf-reaction thathappens at theanode.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughinformation tocalculate the cellvoltage understandardconditions?O YesO NoExplanationCheck02021 McGraw-Hill Education. All Rights Reserved. Tems of Use Pmvacy AccessibMacBook A Answerollowing questions about this cell.Write a balancedequation for thehalf-reaction thathappens at thecathode.eWrite a balancedequation for thehalf-reaction thathappens at theanode.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isD.spontaneous aswritten.Do you haveenoughinformation tocalculate the cellvoltage understandardconditions?O YesNoIf you said it waspossible tocalculate the cellvoltage, do so andenter your answerhere. Round youranswer to 4significant digits.CheckExplanation2021 McGraw-Hill Education. Alt Rights Reserved Tems of Use

In electrochemical series ions are arranged with their increasing order of standard reduction…

A chemist designs a ses these two hait-reactions: half-reaction standard reduction potential 2+ Cu"(aq)+e - Cu (aq) +0.153 V 2 10,(aq)+12 H (aq)+10e L(s)+6H,O(1) +1.195 V !3! Answer the following questions about this cell. Write a balanced 0-0 equation for the half-reaction that happens at the cathode. Write a balanced equation for the

A chemist designs a ses these two hait-reactions: half-reaction standard reduction potential 2+ Cu"(aq)+e - Cu (aq) +0.153 V 2 10,(aq)+12 H (aq)+10e L(s)+6H,O(1) +1.195 V !3! Answer the following questions about this cell. Write a balanced 0-0 equation for the half-reaction that happens at the cathode. Write a balanced equation for the

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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Using the following standard reduction potentials E° = -2.92 V Cs*(aq) + e –→ Cs(s) Cr2*(aq) + 2 e » Cr(s) E° = -0.91 V calculate the standard cell potential and write the cell reaction for a voltaic cell. E°cell = -2.01 V and Cr2+(aq) + 2 Cs(s) → 2 Cs*(aq) + Cr(s) E°c cell = +2.01 V and Cr2*(aq) + 2 Cs(s) → 2 Cs*(ag) + Cr(s) None of these E°cell = +4.91 V and %3D Cr(s) + 2 Cs*(aq) →2 Cs(s) + Cr2+(aq) E°cell = -4.91 V and Cr(s) + 2 Cs*(aq) → 2 Cs(s) + Cr2+(aq)
Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2VO (aq) + 4H* (aq) + Fe (s) → 2VO²+ (aq) + 2H₂O (1) + Fe²+ (aq) + 2+ 2+ Suppose the cell is prepared with 0.564 M VO₂ and 7.14 MH* in one half-cell and 6.21 M VO²+ and 6.29 M Fe² in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. Ú
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4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative
please have the answer to the 3 significant digits.
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…
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn (aq)+Ba (s) Sn (s)+ Ba" (aq) 2+ Suppose the cell is prepared with 4.24 M Sn 2+ in the other. in one half-cell and 2.000 M Ba' Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq) + 12H" (aq)+ 5Co (s) → L, (s)+ 6H,0 (1)+ 5Co" (aq) Suppose the cell is prepared with 6.10 M IO, and 1.61 M H' in one half-cell and 7.06 M Co 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. х10
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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.