Answered: How many amperes of current needs to be…

How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 5.1 g of Sodium (Na) metal at the cathode in 18 minutes. Anow er:

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 3P

See similar textbooks

Related questions

Q: 5.77 of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

Q: If the given statement is true, write T. Otherwise, write F and explain why it is false. 1) The…

A: Given the statement: The electrons in a galvanic cell can be transferred through a wire, making it…

Q: If a constant current of 2.0 amperes is passed through a cell containing Cr3+ for 1.0 hour, how many…

A: Mass of Cr deposited can be calculated using Faraday's first law of electrolysis: Mass deposited=…

Q: Electrolysis of an aqueous magnesium iodide solution at standard conditions would form the following…

A: Given, Electrolysis of an aqueous magnesium iodide solution at standard conditions would form the…

Q: How many amperes of current needs to be passed through molten Sodium chloride to produce 2.4 g of…

A: Faraday's First law, m α Q m = eQ = ect = E96500ct…

Q: A factory wants to produce 1.00 x 10° kg barium from the electrolysis of molten barium chloride.…

A: When electricity is passed through the electrolytic cell, then at the time the amount of substance…

Q: Consider a galvanic cell constructed from the following half cells, linked by a KCl salt bridge. - a…

A: In any galvanic cell, the reduction of that species takes place which has more reduction potential.…

Q: what types of difficulties are to be faced during electrolysis of NaCl ?

A: We acquire hydrogen and chlorine by the electrolysis of aqueous sodium chloride where aqueous sodium…

Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: The mass of three different metal electrodes, each from a different galvanic cell, were determined…

A: The active electrode which is found to lose mass during redox reaction in a cell is termed as anode…

Q: How many seconds are required to produce 8.00g of aluminum metal from the electrolysis of molten…

A: Assume that the required seconds as x. 1 A = 1 C/s. Coulombs generated by 12.0 A in x seconds is 12…

Q: A battery can provide a current of 4.00 A at 1.60 V for 1.00 hr. How much energy (in kJ) is…

A: Given that a current of 4.00 A was provided by battery at 1.60 V. The power can be calculated as…

Q: A factory wants to produce 1.00 x 103 kg barium from the electrolysis of molten barium chloride.…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 1.8…

A: A numerical problem based on electrolysis that is to be accomplished.

Q: A battery can provide a current of 2.20 A at 1.00 V for 8.00 hr. How much energy (in kJ) is…

A: Given information,Battery provides a current 2.20 A at 1.00 V for 8.00 hr.Calculate the power,

Q: What unit is used to measure the magnitude of electrical current? What unit is used to measure the…

A: The unit used to measure the magnitude of electrical current is Amperes.The unit used to measure the…

Q: A factory wants to produce 1.00 × 10 kg barium from the electrolysis of molten barium chloride. What…

A: Electrolysis is a chemistry and industrial process that uses direct electric current (DC) to drive a…

Q: The cathode is the electrode at which oxidation occurs. O True O False

A: We are authorised to call for the one question at a time. Please post the other question separately.

Q: A current of 5.25 A is passed through an aqueous solution of copper(II) nitrate for 71.0 min. How…

A: An swer:- this question is answered by using the simple concept of calculation of mass of a metal…

Q: What amount of Cu (in grams) is deposited at the cathode when a current intained for 15 minutes in a…

A: Faraday's second law of electrolysis explains that when a certain amount of charge is passed, the…

Q: What happens if you interchanged the assigned anode as cathode and the cathode as anode In terms of…

A: In electrochemical cell the electrical energy is form by doing anodic oxidation and cathodic…

Q: Masakatsu plans to create counterfeit gold badges through electroplating. In a filled 500-mL tub, A…

A: Given: Current passed = 875 mA = 0.875 A (Since 1 A = 1000 mA) And…

Q: suppose a current of 0.510 A flows through a copper wire for 281. seconds, calculate how many moles…

Q: (Q98) Electrolysis is being used to plate chromium onto a large plastic surface. If a total of 3.77…

A: Given, mass of Chromium (Cr) = 3.77 g Current (I) = ? Time (t) = ? min Note: molar mass of Cr = 52.0…

Q: Explain the Stoichiometry of Electrolysis?

A: The weights of substances formed at an electrode during electrolysis are directly proportional to…

Q: electrolysis

A: Electrolysis is basically defined as the process in which the electric current is passed through the…

Q: in the electrolysis of water, does the reaction take place at a standard or non standard state?…

Q: A current of 5.37 A is passed through a Cu(NO,), solution for 1.20 h. How much copper is plated out…

A: We will first take out the quantity of charge passes in given time interval. Then we will relate…

Q: Question attached

A: Current is equal to the flow of charge per unit of time. It is denoted by I. Its SI unit is ampere.…

Q: 4. What current is required to deposit on the cathode 5.00 g gold/h from a solution containing a…

A: Current = Charge/Time Q = I/t 1F =96500 C/mol Mass of 1 mole =Molar mass

Q: A current of 0.4 Amps flows for 2 hours through an electrolytic cell containing copper sulphate…

A: This problem can be solved by using Faraday's first law of electrolysis accordingto which weight of…

Q: A(n) cell involves the spontaneous movement of electrons from the anode the cathode. O Nernst O…

Q: what is Faraday's second law of electrolysis ?

A: Electrolysis:Separation of a liquid into its chemical parts by passing direct electric current…

Q: What is the voltage of a galvanic cell that does 788 J of work when 255 Coulomb of charge is…

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: The electrochemical reaction of silver is –

Q: Aluminum plating is sometimes used to reduce corrosion in materials exposed to the outdoors. A…

A: Aluminium sulfate , Al2(SO4)3 is an Electrolytic Substance which on Electrolysis gives aluminium and…

Q: What mass of aluminum can be plated onto an object in 378 minutes at 5.80 A of current?…

A: A numerical problem based on Faraday's law, which is to be accomplished.

Q: What current is used to liberate 213 grams of chlorine, Cl 2 from a solution NaCl if it take 2…

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

Q: If 25 amperes of current flow for 15 minutes through a solution of Sn(NO3)2, how many grams of tin…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: What mass of gold is produced when 15.2 A of current are passed through a gold solution for 25.0 min

A: Given information: Current (I) = 15.2 A Time (t) = 25.0 min

Q: If a 2.5 A current is run through a circuit for 35 minutes, how many coulombs of charge moved…

A: Current is defined as the rate of flow of charge. Write the expression of current. I=Qt where Q is…

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

A: When 96500 coulombs are passed through a solution of NaCl, one mole of chlorine is deposited.

Q: A battery can provide a current of 3.80 A at 3.60 V for 8.00 hr. How much energy (in kJ) is…

A: Given that a current of 3.80 A was provided by battery at 3.60 V. The power can be calculated as…

Q: According to the calculation, the electrolysis formed 0.107 mol M. During this time, 7.00 g M are…

A: Given: No. of mole of (M ) = 0.107 mole Mass of ( M ) = 7 g Find Molar mass of ( M )= ???

Q: What type of reaction takes place in a galvanic cell? nonspontaneous spontaneous

A: A galvanic cell is an electrochemical cell that uses the transfer of electrons in redox reactions to…

Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

Q: during the electrolysis of aqueous solution (NH4) 2SO4, what is the reaction of the environment that…

A: Electrolysis is a technique in which the electric current passes through the solution known as the…

Q: A factory wants to produce 1.00 x 103 kg barium from the electrolysis of molten barium chloride.…

Q: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons…

A: First find number coulombs (C) charge i.e Q = i x t Where Q= charge in coulombs i = current in…

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 amperes of current needs to be
passed through molten Sodium chloride
(NaCl) to produce 5.1 g of Sodium (Na)
metal at the cathode in 18 minutes.
Answer:

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 by step

Solved in 2 steps with 1 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

Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
Is it reasonable to conclude that a potential could be assigned to each half-cell in a voltaic cell, based on these data for three voltaic cells? Explain. Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) cell potential=1.10 V Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) cell potential=1.56 V Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s) cell potential=0.46 V
What is the difference between and ? When is equal to zero? When is equal to zero? (Consider regular galvanic cells as well as concentration cells.)
Determine the overall reaction and its standard cell potential at 25 C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half—cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. 15 the reaction spontaneous at standard conditions?
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) ?
For the standard cell potentials given here, determine the ?G for the cell in k].. (a) 0.000V,n=2 (b) +0.434V,n=2 (c) -2.439 V, n = 1