A piece of electronics requires silver plating. During the plating process, a total of 3.6 g of Ag must be deposited over 5 minutes. What current is required to complete the deposition in the given time? O 350 amps O 5.9 amps O 710 amps O 12 amps

A piece of electronics requires silver plating. During the plating process, a total of 3.6 g of Ag must be deposited over 5 minutes. What current is required to complete the deposition in the given time? O 350 amps O 5.9 amps O 710 amps O 12 amps

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: ctrolyzed by passing a current of 0.500 A through 1.00 L 22SO4 solution for 120 minutes. Determine…

Q: Current is applied to a molten mixture of CuF, FeCl2, and MgI2. Standard reduction potentials can be…

Q: MISSED THIS? Read Section 20.8 (Page). Silver can be electroplated at the cathode of an electrolysis…

A: According to Faraday first Law of Electrolysis " The chemical deposition due to the flow of current…

Q: Lead cans used to store food are made from steel electroplated with a thin layer of lead. The…

A: The voltage required to reduce (to add electrons to the chemical species) at standard conditions is…

Q: Write the balanced equation, including states of matter, for the oxidation half-reaction. 2. Write…

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

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: 19. Balance the net ionic redox equation by the half-reaction method, in acid and base. MnO2(s) +…

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: Write the shorthand notation of the cell in question 3. If the standard reduction potential for…

A: The reaction is spontaneous with negative value of ΔG◦ and positive value of E◦

Q: 22. Consider an electrochemical cell based on the reaction: 2H+ (aq) + Sn (s) Sn2+ (aq) + H2 (g) 22…

A: Here in this question we will apply the nernst equation and see on which factors does the cell…

Q: For the following galvanic cell: Zn(s) + Ni+2(aq) → Zn+2(aq) + Ni(s) A. Of the two half reactions…

A: Since you have posted question with multiple subparts as per guidelines we can answer only three per…

Q: The following electrochemical data may be helpful in answering the question below. Use the table of…

A: Current (i) = 2.1 Ampere Weight of Cr = 0.8 gm

Q: Part A How many grams of chromium metal are plated out when a constant current of 8.00 A is passed…

Q: Which of the following metals can be used to cathodically protect an iron sculpture? Nickel Lead…

Q: Learning Goal: To understand the components and processes of a galvanic cell. A galvanic cell (or…

A: Given cell reaction: Ni(s) + Cu2+(aq) → Ni2+(aq) + Cu(s) We have to find the cathode and the anode…

Q: 22. Consider an electrochemical cell based on the reaction: 2H+ (aq) + Sn (s) → Sn2+ (aq) + H2 (g)…

A: Given: 2H+ (aq) + Sn (s) → Sn2+ (aq) + H2 (g) Which of the following actions…

Q: How long (in minutes) will it take to chromium plate an object of 0.160 m2 to a thickness of 1.30…

A: We have to calculate the time taken in minutes for the deposition.

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

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: The relationship between standard free energy ∆Go and standard electrode potential Eo is: ∆Go=-nFEo…

Q: Write a balanced chemical equation (including states of matter) for an electrochemical cell that has…

Q: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

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

A piece of electronics requires silver plating. During the plating process, a total of 3.6 g of Ag must
be deposited over 5 minutes. What current is required to complete the deposition in the given time?
O 350 amps
O 5.9 amps
O 710 amps
O 12 amps

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

VIEW

Step 2 Faraday's law for electrolysis

VIEW

Step 3

VIEW

Step 4

VIEW

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

According to Standard reduction potentials table on page 164 (OLI), which of the following metals would reduce Sn (tin) from its solution? Sn+2 + 2e Sn O Au (gold) O Fe (Iron) O Pb (lead) O Cu (copper)
Answer the following questions using the data in Appendix L of the textbook. a. Calculate the standard cell potential for a galvanic cell made with Ni and Ag. b. Calculate the standard cell potential for a galvanic cell made with Ni and Zn.
A 20.0 mL sample of effluent contains approximately 10° M of copper ions. At the chosen electrode this generates about 1 nA of current during the deposition step. What length of deposition time would be required to deposit about 2% of the copper? O 13 minutes O 6.5 minutes O 130 minutes O 772 minutes O 26 minutes
Many underground pipes are protected from corrosion by connecting them by a conducting wire to a block of magnesium metal buried close to the pipe. The magnesium protects the iron by acting as a sacrificial anode. Another metal which could also act as the sacrificial anode would be zinc mercury copper O nickel silver
A layer of chromium is electroplated on an automobile bumper by passing a constant current of 40.0 A through a cell that contains Cr3+(aq). How many hours are required to deposit 151 g of chromium? Note: Electroplating is the formation of a metal by the reduction of a metal cation. Select one: a. 32.7 h b. 58.4 h c. 5.84 h d. 3.27 h e. 19.5 h f. 1.95 h
232. Subject :- Chemistry
A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.
If 1.0 Amp of current is used to reduce the following metal ions to metal for a period of 25 seconds, which solution will produce the largest mass of metal? A. 0.2 M Cu2+ B. 0.1 M Ag+ C. 0.5 M Sn4+ D. 0.1 M Cr3+
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.
Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)