Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag+ (aq) +e → Ag(s) What mass of silver plates onto the cathode when a current of 8.2 A flows through the cell for 76 min ? Express the mass in grams to two significant figures.

Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag+ (aq) +e → Ag(s) What mass of silver plates onto the cathode when a current of 8.2 A flows through the cell for 76 min ? Express the mass in grams to two significant figures.

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: A total of 1.740 F of electricity (1 F=1 mol e−) was required to electrodeposit all of the Zn and Co…

A: The mass of each compound is calculated by the number of moles of the compound. The number of moles…

Q: What is the electrical current, in Amperes, that must be applied if 6.50 g Ag is deposited at the…

Q: balance the reaction in acidic solution • identify the species oxidized, the species reduced, the…

A: Species which oxidized is I-. Species which reduced is Pb+4 Oxidizing agent is Pb+4 Reducing agent…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

Q: Silver can be electroplated at the cathode of an electrolysis cell according to the following…

A: Given information:Current (I) = 6.4 ATime (t) = 69 minutes

Q: one process used for electroplating silver, a current of 10.23 A was passed through an electrolytic…

A: Electroplating is a process in which a thin layer of one metal is deposited on another metal surface…

Q: Three electrochemical cells were connected in series so that the same quantity of electrical current…

A: Concept introduction: Faradays second law of electrolysis is explained as when the same quantity of…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

Q: Calculate the mass of Ag metal generated when Ag(NO3)(aq) is electrolysed for 20.5 minutes with a…

Q: A certain metal M forms a soluble nitrate salt MNO 3. Suppose the left half cell of a galvanic cell…

A: To answer questions in problem , we need to determine which electrode will be positive and…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ MnO₂ (s)…

Q: Calculate the mass of cobalt plated onto the cathode of an electrolytic cell by a current of 15.0 A…

Q: A certain metal M forms a soluble nitrate salt MNO 3. Suppose the left half cell of a galvanic cell…

A: To solve this problem, we need to determine the electrode potentials for both half-cells and the…

Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2 Cr³+(aq)…

A: In the given galvanic cell ->Concentration of Cr3+ = [Cr3+(aq)] = 4.87 MConcentration of Ca2+ = […

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: 1 F = 96500 C Moles of chlorine = 1090 / 71 = 15.35 moles Total charge = 2 × 15.35 F = 2 × 15.35…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

Q: Calculate the standard Gibbs free energy change, AGº, in kJ for the following reaction occurring in…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: Given data,Current=29.0ATime=69.0sReaction at cathode;Pb2++2e-→Pb(s)

Q: A current of 2.90 A was applied to an electrolytic cell containing molten CdCl2 for 54 minutes.…

A: We have to calculate the mass of cadmium metal deposited when current passed is 2.90 A for 54…

Q: Cathode: Ag,O (s) + H,O (1) + 2 e 2 Ag (s) +2 OH (aq) Anode: Zn (s) +2 OH (aq) → ZnO (s) + H,O (1) +…

A: In coin / button battery redox reaction take place, where Oxidation state of silver changes from +1…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn²+ (aq)…

A: Given Cell reaction: Sn2+(aq) + Ba (s)---> Ba2+(aq) + Sn (s) From standard electrochemical data,…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: Step 1: Calculate the Total Charge Passed (Q) Q = I t Q = (32.0 A) * (63.0 s)Q = 2016 A-s or 2016…

Q: The reaction occurring in the cell in which Al2O3 and aluminum salts are electrolyzed is Al³+ (aq) +…

A: Given electroyzed reaction-Using current =1.0 X 105 ATotal time=24 hour day =(24 X 60 X60 )second…

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

Q: How long, in minutes, will it take to produce 370.0 g of pure lithium by running a current of 330 A…

A: Given, Current passing = 330 A Mass of Li = 370.0 g Molar mass of Li = 6.94 g/mol

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

Q: Find the voltage of the cell if the right half-cell contains 0.330 M AgNO₃ (aq) and the left…

Q: Standard tables of reduction potentials assume standard conditions, but many electrochemical cells…

A: Using nernst equation, we will calculate cell potential at given concentrations.

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal calculated as follows

Question

<Chapter 20 Problem Set
Exercise 20.100- Enhanced - with Feedback
MISSED THIS? Read Section 20.8 (Page).
Silver can be electroplated at the cathode of an
electrolysis cell by the half-reaction.
Ag+ (aq) + e → Ag (s)
itemView?assignment ProblemID=210282682&offset=next
Part A
Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction:
Ag+ (aq) + e → Ag(s)
m =
Submit
Provide Feedback
с
Request Answer
What mass of silver plates onto the cathode when a current of 8.2 A flows through the cell for 76 min ?
Express the mass in grams to two significant figures.
VE ΑΣΦ
?
<
6.0
g
?) H
ㅏ
14 of 15
Review I Constants I Periodic Table

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: Given data

VIEW

Step 2: Calculation of time in second

VIEW

Step 3: Calculation of mass of silver

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode reaction is below. 2 Cl −(aq) → Cl2(g) + 2 e− How long (in s) will it take to produce 1.09 kg of chlorine if the current is 6.00 102 A?
How many moles of hydroxide ion will be produced at the cathode during the electrolysis of water with a current of 4.52 A for a period of 2.77 minutes? The cathode reaction is 2H₂O + 2e → H₂ + 2OH- mol OH = =
The following spontaneous reaction occurs when metallic zinc is dipped into a solution of copper sulfate. Zn (s) +Cu^ 2+ (aq) ----> Zn^ 2+ (aq) +Cu (s) Describe a galvanic cell that could take advantage of this reaction. What are the half-cell reactions? Make a sketch of the cell and label the cathode and anode, the charges on each electrode , the direction of ion flow, and the direction of electron flow .
4
When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PbSO4) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 80.0 A is fed into a car battery for 63.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol. x10 0.0 X μ 010 3
How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an electrolytic cell, if a current of 23.2 A is passed through an aqueous solution of CUSO4?
Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag^+(aq)+e^-→Ag(s) What mass of silver plates onto the cathode when a current of 7.9 A flows through the cell for 73 min ?
Help with the following question Please round the answer to 3 sig figs
B) Balance the following redox reaction in acidic solution: I03 - (aq) + NO2(g) → NO3 (aq) + I»(s)
4)A galvanic cell is constructed that uses the following half-cell reactions: Cu+(aq) + e−→ Cu(s) I2(s) + 2e−→ 2I−(aq) a)Determine the cell potential for the spontaneous reaction under standard conditions. b)If the cell in part a is operated at 298 K with [Cu+] = 2.5 M and [I−] = 3.5 M, calculate the cell potential. Is the reaction spontaneous under these conditions? Explain. c)If [Cu+] was equal to 1.4 M, at what concentration of I− would the cell have zero potential?