Consider the following voltaic cell (Eigure 1) Figure Fels) Voltmeter Sale bridge IMF IM Ag 1 of 1 Agis) Y What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10? Express your answer with the appropriate units. E-E- Value Submit Part C HÅ E-E- * Incorrect; Try Again; 6 attempts remaining Submit Previous Answers Request Answer What is the change in the cell voltage when the ion concentrations in the anode half-cell are increased by a factor of 107 Express your answer with the appropriate units. μÅ + Value V Request Answer 4 TELEVÍ V

Consider the following voltaic cell (Eigure 1) Figure Fels) Voltmeter Sale bridge IMF IM Ag 1 of 1 Agis) Y What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10? Express your answer with the appropriate units. E-E- Value Submit Part C HÅ E-E- * Incorrect; Try Again; 6 attempts remaining Submit Previous Answers Request Answer What is the change in the cell voltage when the ion concentrations in the anode half-cell are increased by a factor of 107 Express your answer with the appropriate units. μÅ + Value V Request Answer 4 TELEVÍ 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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3 attempts left Check my work Be sure to answer all parts. A voltaic cell consists of a standard hydrogen electrode in one half-cell and a Cu/Cu²+ half-cell. Calculate [Cu²+] when E is 0.180 V. cell x 10 M Enter your answer in scientific notation.
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Score on last try: 0 of 2 pts. See Details for more. You can retry this question below Determine the equilibrium constant, K, for the voltaic cell composed of the following 2 half reactions at 298 K. Sn²+ (aq) + 2e Mn²+ (aq) + 2e Report your answer in the format 2.4E-3. 1.87E-36 Sn(s) Ecell = -0.136 V Mn(s) E= -1.19 V cell Hint: Decide which half-reaction is the reduction reaction and which one is the oxidation reaction by looking at Eº; the oxidation reaction should be reversed, and Er will have the opposite sign. ox 4.0560949048976E+35
Calculate the time needed to operate an electrolytic cell to plate 0.55 g of Z that is running at 138 A given the following reaction. z3 (aq) + 3e - Z(5) Atomic Mass: Z: 195.25 g/mol Round your answer to 2 decimal places.
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Answer#12
A voltaic cell is composed of the following 2 half reactions: Mn²+ (aq) + 2e → > Mn(s) Ecell = -1.185 V Cu+ (aq) + e Cu(s) Eell = 0.521 V Determine the non-standard state Ecell at 298 K when Mn²+ (aq) = 0.158 M and Cu+ (aq) = 0.663 M. → V
A galvanic (voltaic) cell is made using the 2 half cells: Zn2+ (aq) + 2e → Zn(s) E =-.763 V Mg2+ (aq) + 2e - → Mg(s) with Zn(s) and Mg(s) as the electrodes. Answer the questions A. It is the anode. [Select ] B. It is the cathode. [Select] C. Electrons in the wire flow toward it. [Select]. D. Anions from the salt bridge flow toward it. [Select] E. Gains mass. [Select] E = -2.37 V F. Losses mass. [Select]
concentration battery works or not? make the necessary calculations. (E = 0)
sub= 18 help
Pls help me asap. MAke sure your answers from each step are all correct
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