How long will it take to plate out each of the following with a current of 200.0 Ampere? a. 1.0 kg of Cu from aqueous Cu?* solution b. 2.0 kg of Pb from aqueous Ag* solution c. 5.0 mol of Au from aqueous Au³* solution

How long will it take to plate out each of the following with a current of 200.0 Ampere? a. 1.0 kg of Cu from aqueous Cu?* solution b. 2.0 kg of Pb from aqueous Ag* solution c. 5.0 mol of Au from aqueous Au³* solution

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: For the cell at 320 K outlined below, answer the questions. Each cell has a volume of 100.0 ml…

A: Given Cell Au (s) | Au3+ (0.05 M) || Au3+ (1.2 M)|Au Temperature- 320 K Volume- 100.0 ml Current-…

Q: Using 1.0 A of current for 60 s, what metal solution will deposit the highest mass of metal ?…

A: NOTE : There is a typo mistake in the option. Among option a and b, one will have Fe(NO3)3. Hence…

Q: Consider a voltaic cell at 25°C consisting of a Fe Pb(s) electrode immersed in a 1.0 M Pb(NO3)2 SO…

Q: Use the table of standard reduction potentials from your textbook to complete the following table.…

Q: Hi there. I do not understand where I am going wrong. Any help is aappreciated!! Thanks!! Given…

A: Given,Amount of current = 1 ampTime = 1 hourRequired, The solution that would…

Q: None

A: First, you need to find the molar mass of manganese. The molar mass of manganese (Mn) is…

Q: Consider a galvanic cell based in the reaction Fe2+ + Cr2O72– → Fe3+ + Cr3+ in acidic solution.…

Q: What is the standard cell potential for the reaction 3A2+(aqg) + 2X(s) 3A(s) + 2X³+(aq)? a. 0.40 V…

Q: 2. You are given an electrochemical cell where the chemical reaction involves a silver complex, and…

A: Solving question 2b as asked. Calculate the concentration of salt undergoing electrolysis

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: Oxidation occurs at the positive electrode of a standard battery (voltaic cell).

A: In volatic cell also called galvanic cell oxidation occurs at anode.

Q: An electrolytic cell is set up to plate Zr(s) from a solution containing Zr4+(aq). A current of 7.59…

Q: Zn 0.10 60 The diagrams above illustrate the equipment used to electroplate four identical objects…

A: Electrochemistry is the branch of chemistry which studies the change of chemical energy into…

Q: What is the standard electrode potential for a galvanic cell constructed from these two half-cells?…

A: The correct option is (B) 1.20V

Q: 1. A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb²+ half-cell. a. Write balanced…

Q: 6. An example of the type of cell described in question 5 can be represented as Mg(s) Mg (0.025 M)…

A: Given-> Mg(s)/Mg2+(0.025M)//Mg2+(1.5 M)/Mg(s)

Q: From the standard electrode potentials table of the cell: Ca I Ca2+ || Zn2+ I Zn calculate AG°…

A: Ered°, Ca2+/Ca=-2.866 VEred°, Zn2+/Zn=-0.76 VAt anode,Ca→Ca2++2e-At cathode,Zn2++2e-→Zn…

Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.4 kg is attached to a buried…

A: The solution is given below -

Q: alculate the standard potential for this cell. Sn(s) + 2 Ag+ (aq) --> Sn2+ (aq) +2 Ag (s) a.…

Q: An electrochemical cell is set up with the following configuration: Hg|Hg2+||Mn2+|Mn. The solutions…

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: What is the value of the equilibrium constant for the reaction between Al(s) and Cd²+(aq) at 25°C?…

A: Al(s) + Cd2+(aq) ----> At anode (oxidation) -> Al(s) ----> Al3+(aq) + 3e At cathode…

Q: A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 ∘C. The initial…

A: a)Reaction at cathode:Cu2+ + 2e- --> Cu(s) Eocathode = 0.34 VReaction at anode:Pb (s) -->…

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: A student sets up a voltaic cell using a 1 M zinc sulfate solution with a zinc electrode and a 1 M…

A: We need the standard reduction potential values for Zn2+(aq) and Sn2+(aq), which are given below:…

Q: 9. A current of 8.00 amps is passed through a molten solution of Al+3 ions for 40.0 min. How many…

A: Step 1: Step 2:Step 3: Step 4:

Q: 1. The cathode in a galvanic and electrolytic cells is: negative in certain type of cells the site…

Q: 9. How many grams of Cu are plated out from a CuSO4 solution by a current of 7.8 amps flowing for…

A: We have to predict the mass of Cu deposited.

Q: An unknown metal M is electrolyzed. It took 95.5 seconds for a current of 1.60 amp (A) to plate out…

A: Time taken t = 95.5 s Current I = 1.60 A Mass of metal deposited m = 0.175 g We need to find molar…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

How long will it take to plate out each of the following with a current of 200.0 Ampere?
a. 1.0 kg of Cu from aqueous Cu?+ solution
b. 2.0 kg of Pb from aqueous Ag* solution
c. 5.0 mol of Au from aqueous Au³* solution

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

Consider a concentration cell containing two half cells with two Ag electrodes, one with 2.5 M Ag+and one with 2.5 x 10-3 M Ag+. In this case, which of the following statements are true? I. Electrons will flow from the half cell with higher towards that of lower concentration.II. The final concentrations of Ag+in the two half cells will eventually become equal.III. E° = 0 VIV. The cell does not need a salt bridge since silver ions are in both half cells. A) I and II onlyB) II and III onlyC) I and III onlyD) I, III and IV onlyE) II, III and IV only
plz explain step by step in detail :)
A voltaic cell consists of a Pb/Pb?+ half-cell and a Cu/Cu2+ half-cell at 25 °C. The initial concentrations of Pb?+ and Cu?+ are 0.0530 mol L1 and 1.60 mol L-', respectively. Part B What is the cell potential when the concentration of Cu+ has fallen to 0.240 mol L? Pb?+ (ag) +2 e → Pb(s) E° = 0.13 V Express your answer using two decimal places. Cu (ag) + 2 e → Cu(s) E = 0.34 V Ecal = 0.489 V Submit Previous Answers Request Answer X Incorrect; Try Again Part C What are the concentrations of Pb?+ and Cu?+ when the cell potential falls to 0.36 V? Express your answers using two significant figures separated by a comma. ? [Pb* ]- [Cu*] = mol L Submit Request Answer
74. A voltaic cell employs the redox reaction: Sn²+(aq) + Pb(s) Sn(s) + Pb2+(aq) E° cell = 0.010 V Calculate the cell potential, Ecell, at 25°C under each set of conditions. a. [Pb2+] = 0.010 M; [Sn²+] = 0.010 M b. [Pb2+] c. [Pb2+] = = 1.0 × 10 6 M; [Sn²+] = 2.0 M 1.5 M; [Sn2] = 0.010 M
A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell in that time? (F = 96,500 C/mol)
1
Consider the cell described below. Al | Al³+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [A13+] to have changed by 0.46 mol/L. (Assume T= 25°C.) V Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors Supplemental Data
A current of 8.00 amps is passed through a molten solution of Al+3 ions for 40.0 min. How many grams of 1 mol e¹ = 96,500 C aluminum metal are produced? Al = 26.98 g/mol A) 16.1 g B) 5.37 g C) 1.79 g D) 0.0298 g E) 27.0 g Al 3+3 e → Al
1.How many grams of NaCl is present on 5.0 mL of 1.0 % m/V NaCl solution? 2. A zinc bar weighing 3.0 kg is attached to a buried iron pipe to protect the pipe from corrosion. An average current of 0.020 A flows between the bar and the pipe. How many years will be required for the zinc bar to be entirely consumed?
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E° V 'cell * TOOLS х10
H11. Consider the voltaic cell H+ (aq, ?? M) H₂(g, 1 atm)||Cu(s) Cu²+ (aq. 0.1 M). Ecell for this cell at 25 C was +0.360V. What was the pH of the anode solution? A. 0 ABCDE B. C. D. E. 0.89 3.2 7.0 11.7
What is the standard cell potential for the reaction given? 2Ag (s) + Pb²⁺(aq) ⟶ 2Ag⁺(aq) + Pb(s) A. 0.926V B. -0.926 V C. 0.674 V D. 0.463 V E. -0.674 V