Answered: How many seconds are required to…

How many seconds are required to deposit 0.164 grams of magnesium metal from a solution that contains Mg** ions, if a current of 0.620 A is applied.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.26QAP

See similar textbooks

Related questions

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

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

A: As per the given information the balanced chemical cathode half reaction is as follows:…

Q: How many grams of nickel metal will be deposited from a solution that contains Ni²* ions if a…

A: Given,

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

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

A: The Faraday's 1st law of electrolysis is one of the most important law which explains the…

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

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: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

Q: How many seconds are required to deposit 0.143 grams of tin metal from a solution that contains Sn2+…

A: Answer: Since, Sn2+ is getting reduced into Sn, therefore its valency factor will be 2 and its…

Q: se a current of 770. mA flows through a copper wire for 10.0 minutes. Calculate how many moles of…

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

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion 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 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: 3. The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a Cuso,…

A: The Faraday's laws are the main concepts of electrochemistry. The first law shows the connection…

Q: How many seconds are required to deposit 0.101 grams of nickel metal from a solution that contains…

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: Mass of cobalt is calculated as:-

Q: How many seconds are required to deposit 0.168 grams of lead metal from a solution that contains…

A: We have deposit of pb as 0.168g . Current passed is 0.974 A We have to calculate the time required…

Q: How many seconds are required to deposit 0.220 grams of chromium metal from a solution that contains…

A: Given that - Mass of chromium deposited = 0.220 g Current used = 1.10 A Then , from following…

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 manganese metal will be deposited from a solution that contains Mn2* ions if a…

A: Faradays laws of electrolysis:

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

Q: How many seconds are required to deposit 0.270 grams of copper metal from a solution that contains…

A: Given weight of deposited copper metal from a solution(w) = 0.270 g Current applied (I)= 0.828 A =…

Q: How many seconds are required to deposit 0.136 grams of copper metal from a solution that contains…

A: Given, mass of Cu deposited = 0.136 g Current passed = 0.913 A 1 Faraday is the magnitude of charge…

Q: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The metal deposited or liberated is given by the Faraday's first law of electrochemistry which is…

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: How many grams of aluminum metal will be deposited from a solution that contains Al^3+ ions if a…

A: Current = 0.826ampere Time = 55.5 minute = 55.5×60 second (1 minute = 60 second)

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

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

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: many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a current of…

A: Given: Current = 0.974 A Time = 67.4 min = 67.4 x 60 = 4044 sec

Q: How many seconds are required to deposit 0.220 grams of aluminum metal from a solution that contains…

A: The reaction taking place is Al3+ + 3 e- ----> Al (s) Hence moles of electron reacting to form…

Q: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The mass of metal deposited can be given by Faraday's first law of electrochemistry which is - W =…

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

A: The charge carried by one mole of electrons is called one Faraday 1 Faraday = 96485 C The…

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

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

Q: How many seconds are required to deposit 0.221 grams of cadmium metal from a solution that contains…

Q: How many grams of iron metal will be deposited from a solution that contains Fe2+ ions if a current…

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

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

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

A: Given-> Current (I) = 0.640 ampere Time(t) = 32 minutes =32×60 second = 1920 second

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

A: According to Faraday law:- 1F or 96485 c change passes to deposite equivalent mass of any…

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 grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a 0.50 M…

A: · change(Q)=current(i)×time(t)· 1F change passed to cu2+ solution to deposite…

Q: How many seconds are required to deposit 0.263 grams of silver metal from a solution that contains…

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

Q: How many seconds are required to deposit 0.262 grams of chromium 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: How many minutes would it take to deposit all the Al from 225 ml of 0.10 M aluminum nitrate with…

A: The given data contains, Molarity = 0.10 M. Volume = 225 ml. Current = 220 A.

Q: How many seconds are required to deposit 0.150 grams of tin metal from a solution that contains Sn2+…

A: Mass = 0.150 g Current (i) = 0.652 A = 0.652 C/s Time (t) = ?

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

100%

A cvg.cengagenow.com
Tap-Cengage Learni.
OWLV2 | Online teaching a.
Courses
Transfer Course Equivalen.
Homepage
Consider The Fol
[Review Topics]
[References)
Use the References to access important values if needed for this question.
How many seconds are required to deposit 0.164 grams of magnesium metal from a solution that contains Mg** ions, if a current of 0.620 A is applied.
Submit Answer
Retry Entire Group
9 more group attempts remaining
(Previous
Next
Email Instructor
Save and Exit
Cengage Learning | Cengage Technical Support
DII
DD
F10
F11
F12
F4
FS
F8
F9
&
)
4
6
7
8
9
R
Y
P

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

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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 0.0712-g sample of a purified organic acid was dissolved in an alcohol-water mixture and titrated with coulometrically generated hydroxide ions. With a current of 0.0392 A, 241 s was required to reach aphenolphthalein end point. Calculate the equivalent mass of the acid.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Using data from Table 17-1, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+,F,H,H2O,I2,K
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
Why would a sacrificial anode made of lithium metal be a bad choice despite its ELi+/Li=2.07V, which appears to be able to protect all the other metals listed in the standard reduction potential table?
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
Consider the reduction of nitrate ion in acidic solution to nitrogen oxide (Ered=0.964V) by sulfur dioxide that is oxidized to sulfate ion (Ered=0.155V) . Calculate the voltage of a cell involving this reaction in which all the gases have pressures of 1.00 atm, all the ionic species (except H+) are at 0.100 M, and the pH is 4.30.