Suppose a current of 90. A flows through a copper wire for 145. seconds. Calculate how many moles of electrons travel through the wire. Be sure your answer has the correct unit symbol and round your answer to 2 significant digits.

Suppose a current of 90. A flows through a copper wire for 145. seconds. Calculate how many moles of electrons travel through the wire. Be sure your answer has the correct unit symbol and round your answer to 2 significant digits.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 13.98PAE

See similar textbooks

Related questions

Q: Simply by living, an 87.5 kg human being will consume approximately 20.0 mol of 0, per day. To…

Q: The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one…

A: Answer: 174.0

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

A: Faraday’s first law of electrolysis: The mass of the substance deposited at the…

Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

Q: How much time in minutes would it take to deposit 4.01 grams of X (MW 163.10 g/mol) on a cathode in…

A: Faraday's second law states that, the amount of substances deposited by the passage of same amount…

Q: A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some…

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

A: The charge carried by 610A of current in 77 seconds is the product of current and time.q is the…

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

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

A: 1.) First we calculate moles of SC using mass and molar mass. 2.) Then we write a balanced chemical…

Q: Suppose a current of 690 mA is passed through an electroplating cell with an aqueous solution of…

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

A: The reaction at Cathode is Lead sulphate is reduced to Lead. PbSO4 + 2e- ---> Pb + SO4 2-

Q: A large electrolytic cell that produces metallic aluminum from Al2O3 ore is capable of making 250 kg…

A: The total current required for the process of given electrolytic cell is determined as shown below,

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: The element hafnium, Hf, is used in control rods for nuclear reactors and as an insulator for…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction:

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

A: Answer = 0.530 grams

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

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

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

Q: 4.) What mass of silver can be plated onto an object in 45 minutes at 9.0 A of current?

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: 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: 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: A battery can provide a current of 2.20 A at 1.40 V for 10.0 hr. How much energy (in kJ) is…

A: GIVEN: Current = 2.20 A Voltage = 1.40 V Time= 10.0 hr To CALCULATE: Energy (kJ)

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

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

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

A: Given,Current = 59.0 ATime = 66 sec.Molar mass of lead 207.2 g/mol

Q: A student designs an ammeter (a device that measures electrical current) that is based on the…

A: The magnitude of the current in amperes is to be calculated from the given data. Given: Volume of…

Q: If a current of 5.00 A is applied for 96.00 minutes, how many grams of magnesium will be formed?…

A: To find weight of magnesium

Q: Suppose a current of 0.590 A flows through a copper wire for 154. seconds. Calculate how many moles…

A: Given, Current (I) = 0.590 A Time (t) = 154. second Moles of electron transfer through the wire = ?

Q: Solid, metallic chromium can be electroplated from acidic aqueous solutions containing dichromate…

A: Metal electroplated than mass of metal depend current , equivalent weight of metal and time.

Q: Suppose a current of 0.800 A flows through a copper wire for 22.0 minutes. Calculate how many moles…

A: Given: a current of 0.800 A flows through a copper wire for 22.0 minutes. To find: no. of moles of…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: Electrolysis is a process in which current is passed through a substance .In this chemical reactions…

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: Suppose a current of 520. mA flows through a copper wire for 27.0 minutes Calculate how many moles…

A: Given information: Time (t) = 27.0 minutes Current (I) = 520 mA

Q: current

Q: How many grams of Ca metal (atomic mass = 40.08 g/mol) are produced by the electrolysis of CaBr2…

A: From the combination of Faraday's first and second law of electrolysis : W/E = I*t/F Or, W =…

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

Q: How long would it take (in minutes) to reduce 1 mole of each of the following ions using the current…

A: Given information, (a) Fe3+, 2.344 A (b) Cu2+, 25.260 A

Q: What mass of gold can be plated onto an object in 7.29 minutes at 6.39 A of current? Au3+(aq) + 3e-…

A: The amount of gold plated is given below

Q: You pass a 2.5 amp current through an aqueous solution of aluminum nitrate for 5 hours. How many…

A: Aluminium nitrate Al(NO3)3 has Al3+ ions Al3+ + 3 e- -----> Al So to reduce 1 mole Al3+ ions to…

Q: A current of 0.10A has flown through a solution for 3.00 minutes. How many electrons have passed…

A: Given: 1 C = 1 A.s Therefore, for the current of 0.1 A passed through 3.00 minutes, number of…

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: 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: How many grams of Ca metal (atomic mass = 40.08 g/mol) are produced by the electrolysis of CaBr,…

Q: A solution containing a metal ion (M+2, aq) is electrolyzed by a current of 7.8 A. After 15.5…

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

A: According to the Faraday's law of electrolysis, the mass of Substance liberated or deposited at any…

Q: Calculate the standard free-energy change of a voltaic cell with a potential of 0.35 V under…

A: Given data: E0cell = 0.35V no of moles(n) = 2moles of electron formula used: ∆G0 = -nFE0cell Where…

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

Suppose a current of 90. A flows through a copper wire for 145. seconds. Calculate how many moles of electrons travel through the wire.
Be sure your answer has the correct unit symbol and round your answer to 2 significant digits.
?
2021 McGraw Hill LLC AU Rights Reserved Ts of Ui

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

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

If a 2.5 A current is run through a circuit for 35 minutes, how many coulombs of charge moved through the circuit?
Glucose is the major fuel for most living cells. The oxidative breakdown of glucose by our body to produce energy is called respiration. The reaction for the complete combustion of glucose is C6H12O6(s)+6O2(g)6CO2(g)+6H2O(l) If this combustion reaction could be harnessed as a fuel cell, calculate the theoretical voltage that could be produced at standard conditions. (Hint: Use Gf values from Appendix 4.)
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).
Find the potentials of the following electrochemical cell: Cd|Cd2+,M=0.10Ni2+,M=0.50|Ni
Electrochemical Cells II Consider this cell running under standard conditions: Ni(s)Ni2(aq)Cu+(aq)Cu(s) a Is this cell a voltaic or an electrolytic cell? How do you know? b Does current flow in this cell spontaneously? c What is the maximum cell potential for this cell? d Say the cell is connected to a voltmeter. Describe what you might see for an initial voltage and what voltage changes, if any, you would observe as time went by. e What is the free energy of this cell when it is first constructed? f Does the free energy of the cell change over time as the cell runs? If so, how does it change?
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)?
For the scenario in the previous question, how many electrons moved through the circuit?