EvolutionChemisty를 Op늘 17.늘 Ch.들 An:S Sol101b SeaCoLabEmailSearchesCoSolTitii app.101edu.coAppsSchoolSWGOHMSFSWTORAmazonNoodleBillsPossible PurchasesReading listQuestion 10 of 15SubmitConsider the following half-reactions:1:(s) + 2e- →2 1(aq), E°(red) = 0.54 V,Cd2"(aq) + 2 e → Cd(s), E°(red) = -0.40 V.Will the electrochemical cell represented by F| l2 || Cd2- | Cd be galvanic orelectrolytic under standard conditions?A) GalvanicB) ElectrolyticC) Not enough information+

In a galvanic cell spontaneous reaction occurs. In a electrolytic cell non-spontaneous reaction…

Consider the following half-reactions: I2(s) + 2e- → 2 F(aq), E°(red) = 0.54 V, Cd²"(aq) + 2 e- → Cd(s), E°(red) = -0.40 V. Will the electrochemical cell represented by IF | l2 || Cd²" | Cd be galvanic or electrolytic under standard conditions? A) Galvanic B) Electrolytic C) Not enough information

Consider the following half-reactions: I2(s) + 2e- → 2 F(aq), E°(red) = 0.54 V, Cd²"(aq) + 2 e- → Cd(s), E°(red) = -0.40 V. Will the electrochemical cell represented by IF | l2 || Cd²" | Cd be galvanic or electrolytic under standard conditions? A) Galvanic B) Electrolytic C) Not enough information

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 Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following half-cell systems: Ag+(0.010M) + e- --> Ag Eo= +0.80 V Cr3+(O.010M) + 3e- --> Cr Eo= -0.74 V
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
Calculate the reaction temperature of the electrochemical cell described below which measures a potential of 0.313 V. Cu(s) | Cu2+ (0.80 M) || O2(g) (0.98 atm) | H+ (0.047 M), H2O2 (0.92 M) | Pt(s) (Use R = 8.314 J/mol-K; F = 96485 C/mol)
Consider the following voltaic cell at 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? The overall cell reaction is Al3+(0.20 M, ag) Al3*(0.75 M, ag) and Ecell = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) AI3+(0.20 M, ag) and Ecell = +0.0113 V. None of these The overall cell reaction is Al3+(0.20 M, aq) Al3*(0.75 M, ag) and Ecell = +0.0113 V. There is no overall cell reaction and Ecell 0.00 V. %3D The overall cell reaction is Al3+(0.75 M, aq) Als*(0.20 M, aq) and Ecell = -0.0113 V.
(a) Define molar conductivity of a substance and describe how for weak and strong electrolytes, molar conductivity changes with concentration of solute. How is such change explained?(b) A voltaic cell is set up at 25 °C with the following half-cells:Ag+(0.001 M) | Ag and Cu2+(0.10 M) | Cu What would be the voltage of this cell?(E0cell = 0 .46 V)
A 0.04 M sulfuric acid solution was electrolyzed using copper electrodes. A constant current of 4.44 A for 4.2 minutes caused hydrogen gas to be produced at the cathode. Determine the volume of hydrogen gas (in liters, L) produced at 27.8°C and 1.44 atm. |= nF/t F = 96,485 C/mol 1A = 1 C/sec 1V= 1 J/C Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to three (3) decimal places. Answer: 0.199 The correct answer is: 0.099
6. The above diagram shows a Galvanic constructed from Ag|AGNO3(aq) and Ni|Ni(NO3)2(aq) half-cells and the half-cell electrode potentials are as follows: Ag*(aq) + e--> Ag(s); E° = 0.80 V %3! Ni2*(aq) + 2e --> Ni(s); E° = - 0.23 V Calculate the Ecell at 25°C when the electrolyte concentrations are: [Ag*] = 1.3 x %3D 10-4 M and [Ni2+] = 0.10 M. %3D
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
What is the cell potential (EO) for a galvanic cell formed from the following two half-reactions? PbO2(s) + 3 H*(a) + HSO4-(aq) + 2 e-+ PBSO4(s) + 2 E° = 1.690 V %3D H20(1) PbSO4(s) + H*(aq) + 2 e- → Pb(s) + HSO4-(aq) E° = -0.356 V (A) +1.334 V (B) -2.046 V c) +2.046 V D) +2.758 V
Consider the following half-reactions: Half-reaction E° (V) Cl2(g) + 2e" → 2CI'(aq) 1.360v Ni?*(aq) + 2e- Ni(s) |-0.250V Mn2*(aq) + 2e → Mn(s) -1.180V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Mn2*(aq) oxidize Cl'(aq) to Cl2(g)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.
(ii) State which species is the oxidising agent.
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative