Answered: How many grams of aluminum metal will…

How many grams of aluminum metal will be deposited from a solution that contains Al3+ ions if a current of 0.920 A is applied for 68.5 minutes. _____grams

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 109QAP

See similar textbooks

Related questions

Q: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

Q: Part A. How many seconds are required to deposit 0.123 grams of tin metal from a solution that…

A: Faraday's law in electrolysis:

Q: An unknown metal M is electrolyzed. It took 672.8 s for a current of 2.50 A to plate out 0.121 g of…

Q: How many seconds are required to deposit 0.239 grams of manganese metal from a solution that…

Q: Calculate Current or Time How many amperes are required to deposit 0.242 grams of silver metal in…

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: The questions based on Faraday's first law of electrolysis. it states that mass of an element…

Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.08 kg is attached to a buried…

Q: A constant current of 9.25 amperes is passed through a cell containing iridium (III) nitrate,…

A: We have current as 9.250 A , time as 7.57 hrs, deposit of Ir is taking place, we have to calculate…

Q: current of 4.39 A is applied to a CuSO4 solution to deposit copper. Calculate the time it will take…

A: Given that: Current(I) = 4.39A = 4.39 C/s Mass of copper deposited = 1.00×102g = 100g

Q: How many seconds are required to deposit 0.266 grams of cadmium metal from a solution that contains…

Q: n a copper plating experiment in which copper metal is deposited from a copper(II) ion solution, the…

A: Using Faraday's First of electrolysis: w = ZIt Z = Equivalent mass of metal96500w = Molar mass of Cu…

Q: How many grams of aluminum metal will be deposited from a solution that contains Al3+ ions if a…

A: Answer : We have to calculate weight deposited in grams . Explanation : Al3+(aq) + 3e- -> Al(s)…

Q: A baby's spoon with an area of 6.25cm2 is plated with silver from a silver nitrate solution using a…

A: Calculation of Charge: Q=I×t ...... (1) where Q=charge, I =…

Q: How many grams of aluminum metal will be deposited from a solution that contains AlSt ions if a…

Q: How many grams of mercury metal will be deposited from a solution that contains Hg* ions if a…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn2* ions if a current…

A: Given,

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

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A: Mass can be calculated as:-

Q: How many grams of manganese metal will be deposited from a solution that contains Mn2* ions if a…

A: Faradays laws of electrolysis:

Q: A metal was galvanized with zinc using a solution of zinc nitrate, Zn(NO3)2. How much time was…

A: Answer : We have to calculate time to plate zinc on the metal . Using Faraday laws of electrolysis…

Q: 2) How long, in minutes, will it take to plate out 25.0g of Au from a AuCl3 solution if the current…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn2+ minutes. ions if a…

A: I=0.785 amperes t=61.9minutes n = 2 w=ZIt = 65.3 × 0.785× 61.9 ×60 /2× 96500 w =0.986gm

Q: How many seconds are required to deposit 0.145 grams of zinc metal from a solution that contains Zn*…

A: Answer :- t = 447 (s) The time required to deposit 0.145 g of Zn metal from a Zn2+ solution when…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution the…

A: Given: Time = 3.3 hours Current = 17.8 A Atomic mass of copper = 63.5 g/mol

Q: A solution containg 75.0 mg copper was electrolyzed at a constant current of 0.250 A, causing…

A: Faraday's first law : The amount of substance deposited is directly proportional to quantity of…

Q: A current of 0.46 A was passed through a copper (II) sulfate solution using copper electrodes for 16…

A: According to faraday law of Electrolysis:

Q: How many grams of manganese metal will be deposited from a solution that contains Mn2+ ions if a…

Q: A steady current of 5 A is maintained for 120 seconds in CuSO4 solution. How much Cu is deposited…

Q: How many amperes are required to deposit 0.177 grams of tin metal in 872 seconds, from a solution…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn² ions if a current…

Q: How many grams of chromium metal will be deposited from a solution that contains Cr3+ ions if a…

A: Use w=ZIt formula to get answer Z=gm equivalent=molarmass÷charge Mass= 1407.43gm

Q: How many seconds are required to deposit 0.223 grams of lead metal from a solution that contains…

A: Given that, 0.223 grams of lead metal (Pb) is deposited from a solution that contains Pb2+ ions and…

Q: A car bumper is plated with chromium using chromium (III) ions in solution. If a current of 54A…

Q: How many grams of aluminum metal will be deposited from a solution that contains Al3+ ions if a…

A: Faraday's first law of electrolysis states that during an electrolysis reaction the mass of the…

Q: How many minutes are required to deposit 2.12 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: given mass deposited = 2.12 g current = 2.5 A F = 96500 C/mol

Q: How many grams of mercury metal will be deposited from a solution that contains Hg** ions if a…

A: To solve this problem we will use the Faraday law of electrolysis .

Q: How many seconds are required to deposit 0.164 grams of magnesium metal from a solution that…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn+ ions if a current…

Q: Determine the time required to deposit 5.25 g of silver on a surface from a silver nitrate solution…

Q: How many seconds are required to deposit 0.278 grams of manganese metal from a solution that…

A: Electrical charge is defined as the multiplication of current and time. It is measured in coulombs.…

Q: How many seconds are required to deposit 0.252 grams of tin metal from a solution that contains Sn2*…

A: Mass of Sn = 0.252 g Time = ?

Q: How many hours will it take to plate out all the copper in 250 ml of a 0.250 M Cu+ solution using a…

Q: How many minutes are required to deposit 3.77 g Cr from a Cr³⁺(aq) solution

A: We will calculate time for deposit of metal

Q: How many grams of mercury metal will be deposited from a solution that contains Hg ions if a current…

A: Reduction: It is a chemical reaction that is associated with an increase in number of electrons in…

Q: How many seconds are required to deposit 0.262 grams of chromium metal from a solution that…

Q: How many grams of mercury metal will be deposited from a solution that contains Hg2+ ions if a…

A: Given: Current passed = 0.869 A And time taken = 69.2 min = 69.2 × 60 = 4152 s…

Q: How many grams of magnesium metal will be deposited from a solution that contains Mg2+ ions if a…

Q: A current of 0.44A is passed through a solution of ruthenium nitrate causing reduction of the metal…

Q: 13.71 In a copper plating experiment in which copper metal is deposited from a copper(II) ion…

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 many grams of aluminum metal will be deposited from a solution that contains Al³⁺ ions if a current of 0.920 A is applied for 68.5 minutes.
_____grams

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

A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
A current of 0.44 A is passed through a solution of ruthenium nitrate causing reduction of the metal ion to the metal. After 25.0 minutes, 0.345 g of Ru has been deposited. What is the charge on the ruthenium ion, Run+? What is the formula for ruthenium nitrate?
A small part with a surface area of 2.62 cm2 is plated with a gold coating that is 5.00104 mm thick. The density of gold is 19.32 g cm-3. What mass of gold is in this coating? If a barrel plating run has 5000 of these parts in a single barrel, how long would the run take if the current was 15.0 A? (Gold is effectively plated from Au+(aq).)
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
A baby's spoon with an area of 6.25 cm2 is plated with silver from AgNO3 using a current of 2.00 A for two hours and 25 minutes. (a) If the current efficiency is 82.0%, how many grams of silver are plated? (b) What is the thickness of the silver plate formed (d=10.5g/cm3) ?
The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
An irregularly shaped metal part made from a particular alloy was galvanized with zinc using a Zn(NO3)2 solution. When a current of 2.599 A was used, it took exactly 1 hour to deposit a 0.01123-mm layer of zinc on the part. What was the total surface area of the part? The density of zinc is 7.140 g/cm3. Assume the efficiency is 100%.
A current of 0.0100 A is passed through a solution of rhodium sulfate, causing reduction of the metal ion to the metal. After 3.00 hours, 0.038 g of Rh has been deposited. What is the charge on the rhodium ion, Rhn+? What is the formula for rhodium sulfate?
The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
An electrochemical cell is set up using the following unbalanced reaction: Ma+(aq)+N(s)N2+(aq)+M(s) The standard reduction potentials are: The cell contains 0.10 M N2+ and produces a voltage of 0.180 V. If the concentration of Ma+ is such that the value of the reaction quotient Q is 9.32 103, calculate [Ma+]. Calculate wmax for this electrochemical cell.
A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?