A constant curent of 1.20 amp is passed through an electrolytic cell containing a 0.100 M solution of AGNO, and a silver anode and a platimum cathode until 2.48 g of silver is deposited. a. How long does the current flow to obtain this deposit? b. What mass of chromium would be deposited in a similar cell containing 0.100 M Cr** if the same amount of current were used?

A constant curent of 1.20 amp is passed through an electrolytic cell containing a 0.100 M solution of AGNO, and a silver anode and a platimum cathode until 2.48 g of silver is deposited. a. How long does the current flow to obtain this deposit? b. What mass of chromium would be deposited in a similar cell containing 0.100 M Cr** if the same amount of current were used?

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: To produce 1.05 kg of solid potassium from molten KCl, how many hours must 0.818 amps be passed…

A: Electrolytic deposition is the production of a metal from a solution containing its salts by the…

Q: What mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution…

A: Faradays first electrolysis Law states that the quantity of reaction taking place in terms of mass…

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

Q: During the curing of a battery plate, which of the following takes place? A. The active material…

Q: How many moles of chromium would be electroplated by passing a current of 5.2 amperes through a…

Q: a. Balance the following redox reaction in acidic solution (include states s, l, g, aq), show the…

A: Answer: When in a chemical reaction oxidation and reduction both takes place simultaneously then…

Q: 14. Water is electrolyzed by passing a current of 0.500 A through 1.00 L of 1.00M Na2SO4 solution…

A: Using Farday s law of electrolysis and ideal gas equation we can solve this problem. volume = 0.466L…

Q: A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag*…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: For a Manganese-Aluminum cell [Mn2+ + 2e- --> Mn (-1.18V)] [Al3+ + 3e- --> Al (-1.66)] 1 M of both…

A: We have to 1. label anode, cathode 2. write half reactions 3. Write overall reaction 4. Write cell…

Q: Electrolysis of 1.00 g of a copper salt required passage of 0.100 A of current for 123 min for…

Q: Macmillan Learning A current of 3.11 A is passed through a Sn(NO3)2 solution for 1.10 h. How much…

Q: Electrolysis of molten MgCl2 is the final production step in the isolation of magnesium from…

A: In the given question we have to calculate the following from the given redox reaction happens…

Q: A concentration cell made using the reaction of Cu/Cu+2 is measured and has a voltage of 0.022 V at…

A: Answer:- This question is answered by using the simple concept of concentration cell in which both…

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: forms Ni 47. Consider the following diagram of a piece of iron, cathodically protected by magnesium:…

Q: Calculate the mass of silver that can be produced by the electrolysis of 1 mol/L of AgCN(aq) using…

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: To produce gallium, gallium oxide which has Ga(III) ion is being reduced. Hence the electrolysis…

Q: 4.) How long would it take (in min) to plate 29.6 g of nickel from a 1.0 M Ni2* solution using a 4.7…

Q: A technician plates a faucet with Cr metal by electrolysis of aqueous Cr2(SO4)3. If a current of 10A…

A: Electrolysis comprises the current/electricity passage through any electrolytic solution. This…

Q: 23) It took 116 hours to produce 603 g of metal X by performing electrolysis on molten XC13 with a…

A: Faradays first law of electrolysis – During electrolysis of any material, the amount of material…

Q: Hydrogen can be prepared by suitable electrolysis of aqueous rubidium (Rb) salts A. True B.…

Q: What mass of chromium could be deposited from a solution of Cr3+ (aq) using a current of 10.0 A for…

A: Q = IT = 10 A * 10800 sec = 108000 C Q / F = 108000 / 96500 = 1.119 mole e- This is a 3 electron…

Question

100%

A constant curent of 1.20 amp is passed through an electrolytic cell containing a 0.100 M solution of AGNO, and a silver anode and a platimum cathode until 2.48 g of silver is deposited.
a. How long does the current flow to obtain this deposit?
b. What mass of chromium would be deposited in a similar cell containing 0.100 M Cr** if the same amount of current were used?

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 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. (20pts)An electrochemical cell is constructed with a piece of copper wire in a 0.830 M solution of Cu(NO3)2 and a piece of chromium wire in a 0.720 M solution of AgNO3. a. Write a balanced equation for the spontaneous reaction that occurs in this cell b. Calculate the potential at 25°C for the cell. c. Sketch a diagram for this cell. i. Label the anode and cathode. ii. Show the direction of electron flow in the external circuit. iii. Show the direction of movement of nitrate ions. d. Determine the value of AG for the cell. e. Present the short-hand notation for the cell.
23
A current of 0.500 A flows through a cell containing Cd(II) for 10.0 minutes. Calculate the maximum moles of Cd removed from the solution? Assume that the current remains constant. A.) 1,04 mmol B.) 51,8 mmol C. )1,55 mmolD). 25,9 mmol
Consider only the species (at standard conditions), in answering the following questions. Give reason for your answers. (Use data from the Standard Reduction Potential table) Br¯,Br2, H*, H2, La3+, Ca and Cd a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by MnOs in acid? d. Which species can be reduced by Zn(s)?
A battery relies on the oxidation of magnesium and the reduction of Cu*. The initial concentrations of Mg+ and Cut are 1.0 x 10M and 1.5 M, respectively, in 1.0-liter half-cells. a. What is the initial voltage of the battery? b. What is the voltage of the battery after delivering 5.0 A for 8.0 h? c. How long can the battery deliver 5.0 A before going dead?
2. Electrolysis of molten NaCl in a Downs cell is the major isolation step in the production of sodium metal. Assuming that 215 g of Na metal forms, a. How many moles of electrons are required? b. How many coulombs are required? C. How many amps will produce this amount in 9.50 h?
A chromium metal was deposited coming from a solution of Cr+3. The amount of the saidmetal deposited weighs 2.19 g. The process is made possible through a current of 35.2Amperes in electrolyte cell. Determine the following:a. How much charge (in C) is required?b. How long (in min) would it take for the reaction to occur?