A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2 Cr (aq)3Ca (s) -» 2Cr (s)+3 Ca2 (aq) 2+ in the other Suppose the cell is prepared with 5.07 M Cr in one half-cell and 4.07 M Ca Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ato ? OO

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2 Cr (aq)3Ca (s) -» 2Cr (s)+3 Ca2 (aq) 2+ in the other Suppose the cell is prepared with 5.07 M Cr in one half-cell and 4.07 M Ca Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ato ? OO

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 at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2 Cr³+ (aq) +3Ca (s) → 2Cr (s) + 3Ca²+ (aq) 3+ 2+ Suppose the cell is prepared with 4.58 M Cr³+ in one half-cell and 2.50 M Ca²+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 X μ 010
Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Mno, (s) + 4H" (aq)+2Cr*" (aq) → Mn** (ag)+ 2H,0 (1) + 2Cr** (aq) 2+ and 4.41 M Cr" in the other. 3+ Suppose the cell is prepared with 3.06 MH and 5.29 M Cr" in one half-cell and 7.34 M Mn Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. Ox10 ロ·ロ Explanation Check O 2022 McGraw Hill LLC. All Rights Reserve
2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn → Zn²+ze E = 0.76 V If the voltage of the cell is 0.45V at 25°C when [Zn²+] = 1.0 M and PH₂ = 1.0 atm, what is [H+]? 2H+ + 2e- → H₂ E = 0.0V (b) For the voltaic cell described in part (a), find the pH of the cathodic solution when pH2 = 1.0 atm and [Zn²+] = 0.1 M and the E*cell = 0.542 V. (c) What amount of time is needed to plate 2.08 g of copper at a constant current flow of 1.26 A from a 0.1 M CuSO4 solution? Cu²+ze--> Cu(s)
20. A galvanic cell is constructed at 25°C as indicated in the shorthand cell notation: Determine the Eºcell, AG° and Kc. Eºcell = AGO = Au(s) | 1.0 M Au³+ (aq) || 1.0 M Au³+ (aq) | Au(s) Kc = ကိုယ် E° = +1.50 V cat-an
A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at 25 °C, and each compartment has a volume of 227 mL. The cell delivers 0.31 A for 32.1 h. (a) How many grams of Cu are deposited? g Cu
Help with the following question Round the answer to 3 sig figs
|| Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 0 2+ 2+ Cu (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ 2+ Suppose the cell is prepared with 1.39 M Cu in one half-cell and 2.14 M Zn in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 ロ・ロ X μ
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A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 200. mM solution of MSO4 and the right half cell with a 4.00 M 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 20.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 left right x10 X S
A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e → NO(g) + EO red = +0.96 V 2H₂0 (1) Cu2+ (aq) + e → Cut (aq) Ere red= +0.153 V The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] V..
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V ʼred MnO,(aq)+2 H,O(1)+3e MnO,(s)+4 ОН (аq) E=+0.59 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 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.
A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 125. mM solution of MSO4 and the right half cell with a 2.50 M 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. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. left right x10 X Ś