www.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-takeeqF2#3EDVConsider the concentration cell shown below. Calculate the cell potential at 25°C when the concentration of Agin the compartment on the right is the following.F3$4RAg-For each case, also identify the cathode, the anode, and the direction in which electrons flow.a. 0.15 ME =F(Ag]=1.0 MCathode:Anode:F4Cathode:Anode:Direction:b. Calculate the potential when both solutions are 0.49 M in Ag+E =Direction:Show Hint%5TVDIIGVAgCengage Learning | Cengage Technical SupportF5OLO6[Review Topics]YHF67☀UF7J*[References]PrtScn8F8Home(K9F9OEndLF10PPreviousPgUpF11NextSave and Exit4x8:29 PM12/2/2022PgDnF12

Concentration cell is a type of galvanic cell which is constructed by using two electrodes of same…

w.com/ilmn/takeAssignment/takeCovalentActivity.do?locator-assignment-take 1 eq Ag- Consider the concentration cell shown below. Calculate the cell potential at 25°C when the concentration of Ag in the compartment on the right is the following. [Ag]=1.0 M Cathode: Anode: For each case, also identify the cathode, the anode, and the direction in which electrons flow. a. 0.15 M E = [Review Topics] V Show Hint [References] Direction: b. Calculate the potential when both solutions are 0.49 M in Ag+. E = Cathode: Anode: Direction: V Previous Next Save and Exit

w.com/ilmn/takeAssignment/takeCovalentActivity.do?locator-assignment-take 1 eq Ag- Consider the concentration cell shown below. Calculate the cell potential at 25°C when the concentration of Ag in the compartment on the right is the following. [Ag]=1.0 M Cathode: Anode: For each case, also identify the cathode, the anode, and the direction in which electrons flow. a. 0.15 M E = [Review Topics] V Show Hint [References] Direction: b. Calculate the potential when both solutions are 0.49 M in Ag+. E = Cathode: Anode: Direction: V Previous Next Save and Exit

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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nge in 5 on 6 O tion 7 stion 8 estion 9 " Question 10 11 Submit Use the References to access important values if needed for this question. A Fe Fe²+ || Cd²+ | Cd galvanic cell is constructed in which the standard cell voltage is 3.70×10:2 V. Calculate the free energy change at 25°C when 0.863 g of Cd plates out, if all concentrations remain at their standard value of 1 M throughout the process. What is the maximum amount of work that could be done by the cell on its surroundings during this experiment? Submit Answer 5 question attempts remaining AGⓇ Maximum work= X A
3. write a report on the use of zinc as a “sacrificial anode” to minimise the corrosion of iron and steel such as on ships. Use the standard electrode potentials given in question 2 above to predict the cell emf and overall equation for the reaction that would occur in standard conditions between zinc and iron. With ocean-going ships, however, what is the solution in which the two metals are immersed? Is this solution always at an exact concentration of 1 mol dm-3? And in what ways does this real-life situation differ from the standard condition of 25oC / 298K Picture of question 2 is also given
2. For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M)
Calculate the cell potential of a voltaic cell given the following standard potentials: X -> X2+ + 2 e- Eo = -1.69 V Y3+ -> + 3 e- -> Y Eo = 0.94 V Note: Answer in 2 decimal places.
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For the voltaic cell described by the cell reaction below, (1) write the cell diagram, (2) identify which specie is being reduced and which is being oxidized, (3) identify the anode and the cathode, (4) calculate the values of Q, and (5) using the table of standard reduction potentials, show the calculation of the Ecell using the Nernst equation [Ecell = E0cell – (0.0592/n x log Q)]. Zn + Ni+2 (0.10 M) → Zn+2 (0.30 M) + Ni
A voltaic cell is constructed from a standard Mg?+ | Mg half cell (E°red = -2.370 V) and a standard Br, | Br half cell (E°red = 1.080 V). (For all reactions below, use the smallest possible integer coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. Enter electrons as e .) The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is Submit Answer Try Another Version 3 item attempts remaining
A voltaic cell is constructed from a standard Cr+ Cr half cell (E°red = -0.740V) and a standard F2F half cell (E°. red = 2.870V). (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: per) Greek(lower) Arrows Other The cathode reaction is: + elp The spontaneous cell reaction is: The cell voltage is V.
A lithium battery is being developed. Its voltaic cell is constructed based on Li metal electrode and PbsO4 solid electrode. Their standard reduction potentials at 25 °C are given below. E°(Li* (aq) → Li (s)) = -3.040 Volt E°(PbSO4 (S) > Pb (s) + SO42 (aq) = - 0.356 Volt. Which of the following statements is true about this working (spontaneous) voltaic cell? a. The anode is PbsO4 (s) electrode. The standard cell potential of this voltaic cell is E°(cell) = 2.328 Volt O. PBSO4 (s) is a weaker oxidizing agent than Lit. To make a commercial product, the voltaic cell is adjusted to have [Lit] = 2.1 M and [SO42] = 3.5 M. The cell d. potential E under this condition should be less than the standard cell potential E°(cell). e. None of the above
Enter electrons as e". A voltaic cell is constructed in which the anode is a H, H* half cell and the cathode is a Cu|Cu2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: -1 The net cell reaction is: + In the external circuit, electrons migrate v the Cu|Cu2+ electrode v the H, Ht electrode. In the salt bridge, anions migrate v the H2[H* compartment | v the Cu|Cu²+ compartment.
37125200 2001 Type your numeric answer and submit ELYSTES ESTE ISTS SUBS 23033 with all other cell components in place. ASTER PARENGER FAR SERBE 25029031 Hint Figure 18.9 in Section 18.3 illustrates the components of a voltaic cell. PROTERE GEXEMXXXI TOBAS K VEDEREESGESPE030 ESEC Determine the standard cell potential for a voltaic cell made of a Ag strip and an Al strip immersed in 1.0 M aqueous AgNO3 EPHESISSEME and Al(NO3)3 solutions, respectively, DRESEN Revas CHORENIERS POSSEDERDES MOTERIMOSTERONE 273 SOEXPO ETLENS DE ARBAT SERENE BE DIS mom 0 Cannot be empty X 333 EXTERINE SINGIZININISIE BEEB