2. For the cell notation Mg / Mg+2 /| Sn+2/ Sn.а.What is E° for the cell?b. Write the chemical equation for the cell reaction.С.Which electrode is positive?3. For the cell U/U+3 // Ag*/ AgUse the emf of the cell and E° for Ag* / Ag couple to calculate for the U*3 /U half-cell reaction.E° = 2.588 V4. Consider a voltaic cell consisting of a magnesium electrode in contact with 1.0 MMg(NO3)2 anda cadmium electrode in contact with 1.0 M Cd(NO3)2. Calculate E°for the cell and draw a diagram showing the cathode, the anode, and thedirection of electron flow.

An electrochemical cell is generally represented as follows: A∥C Where A represents the process…

Answered: 2. For the cell notation Mg / Mg+2 //…

2. For the cell notation Mg / Mg+2 // Sn+2/ Sn. a. What is E° for the cell? b. Write the chemical equation for the cell reaction. С. Which electrode is positive?

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...

See similar textbooks

Related questions

Q: Use tabulated electrode potentials to calculate AGn for each reaction at 25 °C. a. 2 Fe"(aq) + 3…

A: Given chemical reactions are: Calculate ∆G°rxn for each reaction.

Q: Consider the voltaic electrochemical cell shown to the image. a. Write out the equations for the…

A: a) The half cell reactions taking place are as follows: Anode Cd(s)→Cd2+(aq)+2e-…

Q: An electrochemical cell has a positive standard cell potential buta negative cell potential. Which…

A: Formula: ∆G =∆G°+2.303RT log Q Ecell=Ecell°-0.0591nlog Q For negative value of cell potential, Q…

Q: a. Write the overall cell reaction/cell representation b. Calculate the standard cell potential (Eº)…

A: The half-reactions are – Oxidation or anode half cell reaction - Ca →Ca2++2e-...E∘oxd.=2.87…

Q: Consider the voltaic cell with a standard cell potential of +0.53 V. Ba(s)⎥Ba2+ (0.015 M)⎥⎥ Mg2+…

A: Given cell Ba(s)|Ba2+(0.015 M) || Mg2+(0.05 M)|Mg(s) Standard cell potential Ecell0=+0.53 V R= 8.314…

Q: A concentration cell is an electrochemical cell with identical electrodes in solutions of different…

Q: Al(s) + 3 Ag*(aq) Al*(aq) + 3 A -> A voltaic cell utilizes the reaction above. What is the effect c…

A: ECell = Ecathode - Eanode = Ereduction - Eoxidation Thus we have to 1st identify the cathode…

Q: 80. Consider the concentration cell: Pb(s) Salt bridge containing NaNO3(aq) 2.5 M Pb2+ 5.0 × 10 ³M…

A: Anode is where oxidation occurs, and cathode is where reduction occurs. Oxidation is the process of…

Q: 14. When solid iron reacts with air to produce solid iron (II) oxide, which of the following can be…

A: The objective of this question is to understand the role of iron in the given chemical reaction. In…

Q: In an electrolytic cell using inert electrodes, a current of 5.00 A is passed through a molten…

A: The question is base on the Faraday first law of electricity

Q: A voltaic cell is constructed using electrodes based on the following half reactions: Pb2+ (aq) +…

A: Voltaic cell (or) Galvanic cell: the cell in which chemical energy is converted in to electrical…

Q: Is the reaction spontaneous based on its standard cell potential? a. Yes, because the standard cell…

A: For a spontaneous reaction at standard condition ∆G° must be negative. Also ∆G° = -nFE° n = number…

Q: Super Iron Batteries In 1999, scientists in Israel developed a battery based on the following cell…

A: •Here reaction of iron battery is given. •We have to calculate oxidation number, transferred…

Q: 1. An electrochemical cell comprises two electrodes: (Zn²+/Zn) and (Ag/Ag). Use the standard…

A: Note: As per the guidelines, solution of 1st question has been made and for the expert solution of…

Q: UNIT 9 KEMEDIATION. THI 4. A voltaic cell is constructed using electrodes based on the following…

A: The specie which has high standard reduction potential that tends to reduce itself and oxidize other…

Q: Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0…

A: In an electrochemical cell, the electrical energy is produced from the spontaneous cell reaction at…

Q: Which of the following statements about the operation of a standard galvanic cell made of a Cu/ Cu…

A: Galvanic cell : The cell which converts chemical energy into electrical energy is called galvanic…

Q: a. Write the overall cell reaction/cell representation (balanced equation) b. Calculate the standard…

A: The half-cell reactions for the reaction 1 is represented as follows: Zn(s) → Zn2+(aq)+2e-…

Q: 2 Na* SO, Zn 2+ Sn Sn2+ so 2-

Q: For the voltaic cell indicated by: Sn (s)|Sn²+ (aq)||Fe3+ (aq), Fe2* (aq)|Pt (8) Sketch the cell,…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: Consider a galvanic cell consisting of: Cu2++2e−Cu2++2e- →→ CuCu 0.34 Zn2++2e−Zn2++2e- →→…

A: In an electrochemical cell, electrical energy is produced from the spontaneous cell reaction at the…

Q: Regarding voltaic/galvanic cells: What process occurs at the cathode in a voltaic cell? a. What…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Consider the reaction Br2(l) + 2F-(aq) → 2Br-(aq) + F2(g) at 298. a. Write the cell diagram. b.…

A: The balanced redox reaction is: Br2(l) + 2F-(aq) → 2Br-(aq) + F2(g)

Q: An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a.…

Q: Balance the following redox equation: ____Al(s) + ____Pb2+(aq) → ____Al3+(aq) + ____Pb(s) b. Label…

Q: A concentration cell consists of two Ni/Ni2+ electrodes. One electrode contains 0.15 M Ni²+ and the…

A: Given the Ni2+(aq) concentrations in the half-cells are 0.15 M and 0.95 M

Q: I. Calculate the standard cell potential for each of the following reactions. 2Ag*(aq) + Pb(s) →…

A: A question based on electrolysis that is to be accomplished.

Q: Consider the voltaic cell: Ni(s)|Ni2+ (1.0 M)||H+ (1.0 M)|H2 (1 atm)|Pt(s) Which of the…

Q: In an electrolysis of a solution containing Ni^2+ (aq), metallic Ni (s) deposits on the cathode.…

Q: Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0…

Q: 2. The net equation for a given voltaic cell is: Sn (s) + 2 Agt → Sn²+ + 2 Ag (s) Write the two…

A: The question is based on the concept of electrochemistry.We need to identify half cell reactions and…

Q: Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0…

A: Here we are required to find the anodic and cathodic reaction for the given electrochemical…

Q: a. Given the following standard cell notation, draw and label the electrochemical cell. Be sure to…

Q: 3. For the reaction: Zn(s) + 2Ag (aq)-Zn2(aq) 2Ag(s).. a. Determine the standard cell potential. b.…

A: Standard cell potential: E°cell =E°reduction -E°oxidation Where E°reduction = standard reduction…

Q: 24. Given the electrochemical reaction shown, what is the standard free energy change AG° if E° =…

A: Hence option A is correct that is -311kJ/mol

Q: Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn 2+ and a silver…

A: The electrochemical cell is used to convert chemical energy to electrical energy or it may use…

Q: describe the mass spectrum MASS SPECTRUM to5 100 80 60 40 20 0.0+ 0.0 80 120 160 200 240 40 m/z DA…

Q: 8. Which of the following statements regarding the concentration cell are correct? 1. The standard…

Q: For the following voltaic cell: Fe(s) | Fe^2+(aq, 1.0 M) || Cu^2+(aq, 1.00 M) | Cu(s) a. Draw a…

Q: A voltaic cell consists of a Pb/Pb?+ half-cell and a Cu/Cu2+ half-cell at 25 °C. The initial…

Q: For each of the following; a. Write the overall cell reaction/ cell representation b. Calculate…

A: 1. Zn(s) + Ni+2(aq) → Zn+2(aq) + Ni(s) Writing the overall cell reaction/cell representation

Q: A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell…

A: Given : Current passed = 0.20 A And time = 1 min

Q: 11. What is AGO for the reaction driving the following voltaic cell? Co (s) | Co²+ (aq) || Mn³+…

Question

100%

2. For the cell notation Mg / Mg+2 /| Sn+2/ Sn.
а.
What is E° for the cell?
b. Write the chemical equation for the cell reaction.
С.
Which electrode is positive?
3. For the cell U/U+3 // Ag*/ Ag
Use the emf of the cell and E° for Ag* / Ag couple to calculate for the U*3 /U half-
cell reaction.
E° = 2.588 V
4. Consider a voltaic cell consisting of a magnesium electrode in contact with 1.0 M
Mg(NO3)2 anda cadmium electrode in contact with 1.0 M Cd(NO3)2. Calculate E°
for the cell and draw a diagram showing the cathode, the anode, and the
direction of electron flow.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?
A cell is constructed by immersing a strip of silver in 0.10 M AgNO 3 solution and a strip of lead in 1.0 M Pb(NO 3) 2 solution. A wire and salt bridge complete the cell. What is the potential of the silver electrode in the cell? O a. 0.80 V O b. 0.83 V O C. 0.88 V O d. 0.86 V e. 0.74 V
Consider the reaction below:2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a. Calculate the equilibrium constant for this reaction.b. Calculate the standard cell potential for this reaction.
3. For the reaction: Zn(s) + 2Ag+ (aq) → Zn+2(aq) 2Ag(s). a. Determine the standard cell potential. b. Is the reaction spontaneous? If yes, write the cell notation.
3. Calculate the free energy, AG°, for each electrochemical cell given the following information and determine if the reaction is spontaneous or nonspontaneous. T= 298 K a. E cell =+ 2.10 V, n= 2 b. Каg— 2.2 х 10-3 c. E cell =- 0.677 V, n = 3 =
78. A voltaic cell consists of a Pb/Pb2 half-cell and a Cu/Cu2" half- cell at 25 C. The initial concentrations of Pb and Cu are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential? b. What is the cell potential when the concentration of Cu2" has fallen to 0.200 M? c. What are the concentrations of Pb- and Cu" when the cell potential falls to 0.35 V?
Qd 125.
5. Consider the reaction, Li+2Br → Brz+Li What is the standard potential for this reaction? For the electrochemical cell in which this reaction takes place which electrode is negative electrode? 6. A 5.2A-current posses a bulb. Find the charge in coulombs used by the lamp in 8s. 7. How long has a current of 5 amperes to be applied through a solution of copper nitrate to coat a metal surface of 30 cm² with 0.008 cm thick layer?
6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which [Cu²+] = 5.9 x 10-4 M? Ecell = V b. The copper electrode is placed in a solution of unknown [Cu²+ ]. The measured potential at 25°C is 0.222 V. What is [Cu²+ ] ? (Assume Cu²+ is reduced.) [Cu²+] = M
Zn(s) + 2 H*(aq) → Zn²*(aq) + H2(g) 1. What is the effect on the cell potential of a voltaic cell wi h the above reaction when: The pressure of H2 gas is increased in the cathode. c. Sodium hydroxide is added to the cathode half-cell decreasing the [H"]. а. b. Zinc nitrate is added to the anode d. The surface area of the anode is doubled. half-cell.
Consider a voltaic cell that can be described like so. It is set up at standard conditions. A gold electrode is in contact with Au(NO3)3 (aq) and a lead electrode in contact with Pb(NO3)2 (aq) at 25 degrees C. Write true or false next to each of the following statements regarding the voltaic cell. I. Adding H20 to the lead half-cell will increase the measured cell potential. II. A salt-bridge is used to prevent charge buildup in the half-cells. III. This will result in the production of Pb2+ ions.