A 0.04 M sulfuric acid solution was electrolyzed using copper electrodes. A constant current of 4.44 A for 4.2 minutes caused hydrogen gas to be produced at the cathode. Determine the volume of hydrogen gas (in liters, L) produced at 27.8°C and 1.44 atm. | = nF/t F = 96,485 C/mol 1A = 1 C/sec 1V=1 J/C Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to three (3) decimal places.

A 0.04 M sulfuric acid solution was electrolyzed using copper electrodes. A constant current of 4.44 A for 4.2 minutes caused hydrogen gas to be produced at the cathode. Determine the volume of hydrogen gas (in liters, L) produced at 27.8°C and 1.44 atm. | = nF/t F = 96,485 C/mol 1A = 1 C/sec 1V=1 J/C Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to three (3) decimal places.

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: An unknown metal M forms a soluble compound, M(NO3)3. A solution of M(NO3)3 is electrolyzed. When a…

A: The deposition is M+3 (aq) + 3e– ------> M (s)Number of moles of electrons = 3 × number of moles…

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

Q: A solution of NaCl in water was electrolyzed with a current of 6.51 A for 23.0 min. How many…

A: Answer:Here:

Q: A constant current of 1.6 A is used to precipitate copper at the cathode and oxygen at the anode of…

A: value of constant current = 1.6 A Time = 30.4 minutes cathode - copper Anode - oxygen

Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: Amount of charge (Q) = I . t where I = current and t = time

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

Q: You have a 10.0 cm diameter sphere that you would like to have plated with gold metal. How long…

A: V_uncoated = (4/3)πr^3 = (4/3)π(5.00 cm)^3 = 523.33 cm^3 (diameter=10/2=5cm) Since the coating is…

Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

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: According to the reaction, Ag+ (aq) + e- --> Ag(s), silver is deposited. For 30.0 minutes, a 0.800A…

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: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

A: Given The amount of current (I) is 2.15 A The time is 2.2 hours The density of zinc is 7.410 g/cm3…

Q: What current must be supplied to deposit 4.77 g of gold from a solution of AuCl 3 in 27.2 min?

Q: 3.53 L of 0.362 M solution are electrolyzed (Cu is plated out of solution as metal.) A current of…

A: NOTE: Assuming that the solution contains Cu2+ ions and the concentration data given is for the Cu2+…

Q: A current of 2.90 A was applied to an electrolytic cell containing molten CdCl2 for 54 minutes.…

A: We have to calculate the mass of cadmium metal deposited when current passed is 2.90 A for 54…

Q: Aluminum(III) ion (Al 3+) is reduced to solid aluminum at an electrode. If a current of 2.75 amperes…

Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

Q: What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given ,

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

Q: An aqueous solution of an unknown salt of molybdenum is electrolyzed by a current of 2.50 A passing…

Q: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A mass of…

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: The electrolysis of a copper sulfate solution to get copper metal is carried out using a current of…

A: According to Faraday’s first law of electrolysis, the mass of the element deposited is directly…

Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: According to Faraday's 1st law weight of the substance from in each electrolyte W = ZIt where , W…

Q: A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.…

A: Given: Current, i=0.80 A Time, t=2.5 hours Molar mass of cadmium=112.40 One Faraday=96,500 coulombs

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

A 0.04 M sulfuric acid solution was electrolyzed using copper electrodes. A constant current of 4.44 A for
4.2 minutes caused hydrogen gas to be produced at the cathode. Determine the volume of hydrogen gas (in
liters, L) produced at 27.8°C and 1.44 atm.
|= nF/t
F = 96,485 C/mol
1A = 1 C/sec
1V= 1 J/C
Do not include units in your answer, If you round during your calculations make sure to keep at least 3
decimal places. Report your answer to three (3) decimal places.
Answer: 0.199
The correct answer is: 0.099

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

The gold plating of a ceramic figurine requires a total of 4.19 g of solid gold. If the current being used is 11.0 amperes, how many minutes will it take to plate the gold figurine? You may assume that there is a sufficient concentration of gold cation to complete the process.
A factory wants to produce 1.00 x 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 5.00 h to accomplish this? Current = A
A current of 5.55 A is passed through a Cu(NO3)₂ solution for 1.90 h. How much copper is plated out of the solution? mass of copper:
How many moles of hydroxide ion will be produced at the cathode during the electrolysis of water with a current of 4.52 A for a period of 2.77 minutes? The cathode reaction is 2H₂O + 2e → H₂ + 2OH- mol OH = =
1. How long it takes to deposit 20.4 grams of gold (197 g/mol) when 5.6 ampere current was passed (aq) + 3e → Au(s) through its Au*3 aqueous solution? Au*3 F = 9.65 x 104 Coulombs/moles of es 2. Use the following information, calculate the molar mass of metal “X" and use the periodic table to identify the metal: When 1.24 amps current passed thru it's XCI aqueous solution for 1.5 hours, 5.93 grams of metal X was deposited. {keep in mind the CI-1 has -1 charge and molar mass of XCI = mass/number of moles so first calculate the mass then molar mass}
Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the cathode. Calculate the time it takes to deposit 0.34 gram of gold, passing a current of 0.10 amperes. (1 faraday = 96,485 coulombs)
A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl₂ for 15.5 h. What mass of Mg is produced? g
Thomas Edison invented an electric meter that was nothing more than a simple coulometer, a device to measure the amount of electricity passing through a circuit. In this meter, a small, fixed fraction of the total current supplied to a household was passed through an electrolytic cell, plating out zinc at the cathode. Each month the cathode could then be removed and weighed to determine the amount of electricity used. If 0.25% of a household’s electricity passed through such a coulometer and the cathodeincreased in mass by 1.83 g in a month, how many coulombs of electricity were used during that month?
What mass of gold is produced when 14.9 AA of current are passed through a gold solution for 28.0 minmin ?
A battery can provide a current of 3.80 A at 3.60 V for 8.00 hr. How much energy (in kJ) is produced?
How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60g of calcium from molten CaCl2?
The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a CUSO, solution. From this information, calculate the molar mass of copper.