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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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)
1 2 B A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown: Co2(aq) + 2e Co(s) E° -0.28 volt; Cd2+ (aq) + 2e-Cd(s) E°--0.42 volt. What is the standard free energy change in kJ for the cell reaction of this galvanic cell? Report your answer in whole number. Do not put unit in your answer. Type your answer...
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
Two half-reactions are shown with their standard cell potentials. If a galvanic cell is constructed using them, which electrode would be the anode, and what would the cell potential be? Cd2* (aq) + 2e – Cd(s); E=-0.40 V Cr3+ (aq) + 3e → Cr(s); E=-0.74 V Oa. Cadmium, -0.34 V Ob. None of the other options Oc. Cadmium, -1.14 V Od. Chromium, -1.14 V Oe. Chromium, 0.34 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.
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.
The cell notation for the Galvanic cell is Cd(s)/Ca2+l2(s)/I" The Standard Reduction Potential are as follows: E°Ca2+/cd = -0.403 V; E12/1 = 0.5355 v Calculate the standard cell potential If the Cadmium ions have a concentration of 0.010 M and the iodide ions have a concentration of 0.020 M, calculate the electromotive force (EMF) of the cell. The Gibbs Free Energy of the cell is
(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
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 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.
What is the balanced equation for the galvanic cell reaction expressed using the following shorthand notation? Mg (s) | Mg2+ (aq) || Cl2 (g) | Cl– (aq) | C (s)