MISSED THIS? Watch KCV 19.6; Read Section 19.6. You can click on the Review link to access the section in your eText An electrochemical cell is based on the following two half-reactions: Part A Compute the cell potential at 25°C. Express the cell potential in volts to three significant figures. Ecell Oxidation: Pb(s)→→ Pb²+ (aq, 0.22 M) +2e E-0.13 V Reduction: MnO,- (aq, 1.25 M) + 4H (aq, 2.2 M) +3e MnO₂ (s) + 2H₂O(1), E = 1.68 V VG ΑΣΦΑ +1.85 Submit Previous Answers Request Answer V

MISSED THIS? Watch KCV 19.6; Read Section 19.6. You can click on the Review link to access the section in your eText An electrochemical cell is based on the following two half-reactions: Part A Compute the cell potential at 25°C. Express the cell potential in volts to three significant figures. Ecell Oxidation: Pb(s)→→ Pb²+ (aq, 0.22 M) +2e E-0.13 V Reduction: MnO,- (aq, 1.25 M) + 4H (aq, 2.2 M) +3e MnO₂ (s) + 2H₂O(1), E = 1.68 V VG ΑΣΦΑ +1.85 Submit Previous Answers Request Answer V

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 hypothetical standard half-cell potentials listed below to calculate the standard cell potential in units of V for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)3 Cl 2(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe 3+(aq)Cl 2(g) + 2 e⁻ → 2 Cl⁻(aq) E° = +1.73 VFe 3+(aq) + 3 e⁻ → Fe(s) E° = - 0.14 V
A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.50 M solution of MSO, and the right half cell with a 25.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 40.0 °C. left Which electrode will be positive? x10 O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. necessary, and round it to 2 significant Be sure your answer has a unit symbol, digits.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential CrO2−4 (aq)+4H2O(l)+3e−→ CrOH3(s)+5OH−(aq) =E0red−0.13V Cl2(g)+2e−→ 2Cl−(aq) =E0red+1.359V 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 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. Be sure your answer has the correct number of significant digits. V
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
A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a cell potential of 0.763 V. Calculate the maximum electrical work generated when 17.0 g of zinc metal is consumed. Maximum electrical work-
A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: Cr(s) + 3 Ag*(aq) → Cr³*(aq) + 3 Ag(s) Which of the multiple choices correctly describes how the cell emf changes when a change is made to the cell? Ca) Adding water to the anode compartment makes the cell emf less positive. C b) Increasing the size of the silver electrode makes the cell emf stay the same. C C) Adding a solution of 1.0 M AGNO, to the cathode compartment makes the cell emf more negative. C d) Adding Na,s to the anode compartment to precipitate chromium sulfide makes the cell emf less positive. Ce) Adding a solution of 5 M Ag* to the cathode compartment makes the cell emf stay the same.
MnO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify the oxidizing agent and anode. C) standard cell potential? D) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?
-3 M solution of Cu(NO3)2. The other half-cell consists of a zinc electrode in One half-cell in a voltaic cell is constructed from a copper wire electrode in a 3.9 x 10 a 0.45 M solution of Zn(NO3)2 . Calculate the cell potential. You may need to use the following data: Zn²+ (aq) + 2 e¯ → Zn(s) E° = -0.763 V Cu²+ (aq) + 2 e¯ → Cu(s) E° = +0.337 V Potential = V
3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O
Consider the following half reactions: M²+ (aq) + 2e (aq) → M(S) X³+ (aq) + 3e (aq) →→→→→→X(s) Eº=-0.4 Eº=-0.7 Calculate the overall cell potential for the overall spontaneous redox reaction. Give your answer to one decimal place.
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