A chemist designs a galvanic cell that uses these two half-reactions:half-reactionstandard reduction potential2+Zn (aq)+2e→ Zn(s)=-0.763 VredMnO2(s)+4 H (aq)+2e2+Mn" (aq)+2 H,O(1)E=+1.23 VredAnswer 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 tocalculate the cellvoltage underYesI Don't KnowSubmit02022 McGraw Hill LLC. All Rights Reserved equation for thehalf-reaction thathappens at theanode.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughinformation toO Yescalculate the cellvoltage understandardO Noconditions?If you said it waspossible tocalculate the cellvoltage, do so andenter your answerhere. Round youranswer to 3significant digits.I Don't KnowSubmit2022 McGraw Hill LLC. AllRights

The addition of electrons or decreases in the oxidation state is known as a reduction reaction and…

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e → Zn(s) E=-0.763 V 'red MnO2(s)+4 H (aq)+2e 2+ - Mn (aq)+2 H,O(1) E=+1.23 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that O-0 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 calculate the cell voltage under O Yes

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e → Zn(s) E=-0.763 V 'red MnO2(s)+4 H (aq)+2e 2+ - Mn (aq)+2 H,O(1) E=+1.23 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that O-0 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 calculate the cell voltage under O Yes

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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Use the standard reduction potentials given below to predict if a reaction will occur between Zn(s) and Cl2(g), when the two are brought in contact via standard half-cells in a voltaic cell. | Cl2(g) + 2e¯¯ →2C1¯¯ (aq) E Zn2+ = 1.360 V red (aq) + 2e → Zn(s) E = = -0.763 V red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + +
A galvanic cell is powered by the following redox reaction: 2+ + 3 Cu²+ (aq) + Cr(OH)3(s) + 5OH¯(aq) → 3 Cut (aq) + Cro (aq) + 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 V ロ→ロ X 5
A galvanic cell is powered by the following redox reaction: 2+ MnO₂ (s) + 4H* (aq) + 2 Br¯ (aq) → Mn²(aq) + 2 H₂O(1) + Br₂(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 = = Ov ローロ 0
O ELECTROCHEMISTRY Analyzing a galvanic cell A galvanic cell is powered by the following redox reaction: 3 Br₂(1) + 2 Cr(OH)3(s) + 10OH (aq) - → 6 Br (aq) + 2 CrO (aq) + 8 H₂0(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 E = OV ローロ é X Do ?
Cr(s) Cr(NO3)3 A Voltaic Cell NaCl(aq) Pb(s) Pb(NO3)2 Cr³+ (aq) + 3 eCr (s) E° = -0.41 V Pb²+ (aq) + 2 e¯¯ → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb2+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. O Placing some Cr(s) in a solution containing Cr³+ ions. O Placing some Pb(s) in a solution containing Pb³+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?
Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and Cl₂ (g), when the two are brought in contact via standard half-cells in a voltaic cell. Cl₂(g) + 2e → 2Cl(aq) = 1.360 V red = -0.280 V Co²+ (aq) + 2e → Co(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
A galvanic cell is powered by the following redox reaction: 2 NO(g) + 2 H₂O(l) + Zn²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. + 2H¹ (aq) + Zn(s) 2 HNO₂(aq) + 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 E = -OV ローロ e X ¹0 c.
Consider the reaction: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) What is the half-cell reaction for reduction? Multiple Choice О Fe(s) -> Fe2+(aq) + 2 e- Cu2+(aq) + 2 e-→ Cu(s) О Cu(s) → Cu2+(aq) + 2e- Fe(s) + 2 e-→ Fe2(aq)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction + 21O3(aq)+ 12 H¹ (aq)+10e¯ Cl₂(g) +2e 1₂(s) + 6H₂O(1) → 2 C1 (aq) standard reduction potential E=+1.195 V 'red E 70 = +1.359 V red
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ MnO2(s)+4H (aq)+2e → Mn (aq)+2 H₂O(1) 2+ Zn(aq) + 2e ->>> Zn(s) standard reduction potential E = +1.23 V red = -0.763 V red 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 spontaneous as written. ☐ Do you have enough O Yes information to calculate the cell voltage under standard conditions? O No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 significant digits. Ον ローロ e x10 ×
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V
A galvanic cell has copper cathode and zinc anode. Given the data below, calculate the standard cell potential of this galvanic cell. * Reduction Half-Reactions Cu*2 (ag) + 2e → Cu (s) Zn*2 (ag) + 2e → Zn (s) Reduction Potential 0.340 V - 0.763 V Your answer