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A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H (aq) +5e Cl₂(g) +2e Write a balanced equation for the half-reaction that 0 happens at the cathode. Answer the following questions about this cell. 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 half-reaction information to calculate the cell voltage under standard conditions? 10 Yes 2+ Mn²+ (aq) + 4H₂O(1) 2 C1 (aq) O No standard reduction potential "red = +1.51 V Ered = +1.359 V ローロ e X

A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H (aq) +5e Cl₂(g) +2e Write a balanced equation for the half-reaction that 0 happens at the cathode. Answer the following questions about this cell. 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 half-reaction information to calculate the cell voltage under standard conditions? 10 Yes 2+ Mn²+ (aq) + 4H₂O(1) 2 C1 (aq) O No standard reduction potential "red = +1.51 V Ered = +1.359 V ローロ e X

Chemistry
Chemistry
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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
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A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H(aq) +5e Cl₂(g) +2e 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. Answer the following questions about this cell. 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? half-reaction 0 0 Yes Mn²+ (aq) + 4H₂O(1) →Mn²+, 2 C1 (aq) No standard reduction potential Eº 'red = +1.51 V E=+1.359 V red ロ→ロ X 0x19 S
Transcribed Image Text:A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H(aq) +5e Cl₂(g) +2e 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. Answer the following questions about this cell. 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? half-reaction 0 0 Yes Mn²+ (aq) + 4H₂O(1) →Mn²+, 2 C1 (aq) No standard reduction potential Eº 'red = +1.51 V E=+1.359 V red ロ→ロ X 0x19 S
Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Yes No ☐v
Transcribed Image Text:Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Yes No ☐v
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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 information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. 2+ MnO4 (aq) + 8H¹ (aq) + 5e¯¯ → Mn²+ (aq) + 4H₂O(1) 2C1 (aq) 2MnO4 (aq) + 16H*(aq) + 10Cl - (aq) → 2Mn²+ (aq) + 8H₂0 (1) + 5C1₂ (aq) Yes No Cl₂(g) + 2e 0.15 V ロ→ロ lo e X x10 Ś
Transcribed Image Text: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 information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. 2+ MnO4 (aq) + 8H¹ (aq) + 5e¯¯ → Mn²+ (aq) + 4H₂O(1) 2C1 (aq) 2MnO4 (aq) + 16H*(aq) + 10Cl - (aq) → 2Mn²+ (aq) + 8H₂0 (1) + 5C1₂ (aq) Yes No Cl₂(g) + 2e 0.15 V ロ→ロ lo e X x10 Ś
Try Again Your answer is incorrect. • Row 3: Your answer is not a chemical equation in standard form. A chemist designs a galvanic cell that uses these two half-reactions: + MnO (aq) +8H (aq) +5e Cl₂(g) +2e Write a balanced equation f half-reac Answer the following questions about this cell. half-reaction happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. 2+ → Mn (aq) + 4H₂O(1) 2 C1 (aq) Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as standard reduction potential E=+1.51 V red 2C1 (aq) Cl₂(g) + 2e -0 2+ GMnO4 (aq) + 8H˚ (aq) + 5e¯ → Mn+ (aq) + 4H₂0 (1) E 'red = + 1.359 V 2 MnO4 (aq) + 16H* (aq) + 10C1 - (aq) → 2Mn²+ (aq) + 8H₂0 (1) + 5C1₂ (aq) ロ→ロ X x10
Transcribed Image Text:Try Again Your answer is incorrect. • Row 3: Your answer is not a chemical equation in standard form. A chemist designs a galvanic cell that uses these two half-reactions: + MnO (aq) +8H (aq) +5e Cl₂(g) +2e Write a balanced equation f half-reac Answer the following questions about this cell. half-reaction happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. 2+ → Mn (aq) + 4H₂O(1) 2 C1 (aq) Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as standard reduction potential E=+1.51 V red 2C1 (aq) Cl₂(g) + 2e -0 2+ GMnO4 (aq) + 8H˚ (aq) + 5e¯ → Mn+ (aq) + 4H₂0 (1) E 'red = + 1.359 V 2 MnO4 (aq) + 16H* (aq) + 10C1 - (aq) → 2Mn²+ (aq) + 8H₂0 (1) + 5C1₂ (aq) ロ→ロ X x10
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