Part A If a water electrolysis cell operates at a current of 7.9 A, how long will it take to generate 27.0L of hydrogen gas at a pressure of 23.0 atm and a temperature of 24 C? R0.08206 Latm mor K t6.78 hr Submit Previoun Answer Reauest Answet

Part A If a water electrolysis cell operates at a current of 7.9 A, how long will it take to generate 27.0L of hydrogen gas at a pressure of 23.0 atm and a temperature of 24 C? R0.08206 Latm mor K t6.78 hr Submit Previoun Answer Reauest Answet

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: A certain half-reaction has a standard reduction potential Ered=-0.97 V. An engineer proposes using…

A: Given data is certain half reaction has a standard reduction potential E0red = -0.97VAn engineer…

Q: O The utandard reduction potential qor sn 24 and Ay 3t are -0.14 and † 1.50 V reupectively. Ca…

A: Given: ESn2+|Sno=-0.14 VEAu3+|Auo=+1.50 V

Q: 7. How long has a current of 5 amperes to be applied through a solution of copper nitrate to coat a…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: In an electrochemical cell, Q = 0.010 and K = 855. What can you conclude about Ecell and Ee? a) Ecel…

A: The conclusion about Ecell and Eocell has to be given,

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

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: Consider a cell reaction at 25oC where n=3. 7. Consider a voltaic cell at 25oC in which the…

A: The nernst equation is a relation between electrode potential of a cell and standard electrode…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 19…

Q: An electrolytic cell is set up to plate Zr(s) from a solution containing Zr4+(aq). A current of 7.59…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 12…

A: According to faraday first law Mass of the substance deposited at the electrode is directly…

Q: An electrolysis cell producing Aluminum metal from Al3+ ions runs for 87 minutes at a current of 4.9…

A: Given -> Time(t) = 87 minutes= 87 × 60 seconds= 5220 s (1 minute = 60 seconds) Current (i) =…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 15…

A: Given : Current (I) = 2.6 A Time(t) = 15 min = 900 sec Atomic mass of Z = 182.54 g/mol

Q: surrounded by a 0.834 mol/L solution of ZnCl₂. The second half cell is a standard hydrogen electrode…

A: Since you have asked a question with multiple subparts, we will answer only the first three subparts…

Q: In the electrolysis of water, how long will it take to produce 145.0L of Hz at 1.0 atm and 273…

A: we know volume occupied by hydrogen gas = (weight of hydrogen gas /mol. mass of hydrogen) *22.4 l…

Q: 2. The following cell is set up: ano 2. The following cell is set up: Porous Barrier ly pH - 10.0…

Q: A current of 0.950A passed for 21.0min through a CuSO4 solution. Calculate the amount of copper…

Q: Propose a metal cathode for an electrochemical battery with an anode Tin (2+) using the standard…

A: Since at cathode reduction takes place and at anode oxidation. Hence the reaction taking place at…

Q: How many grams of bromine would be collected after 25 minutes of electrolysis of a molten sample of…

Q: How long will it take to plate out each of the following with a current of 100.0 A? 1.0 kG Al from…

A: 1) The time taken to plate out 1.0 kg of Al from aqueous Al3+ can be calculated as follows: where w…

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…

A: According to Faraday’s first law, the mass of the substance (m) deposited or liberated at any…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 17…

Q: Redox Reaction Half-cell Half-cell Reaction E0oxidatio EOreductio EOredox Spontaneo us? Reaction…

A: Here we are required to find the standard cell potential of the given electrochemical reaction.

Q: A constant current of 5.29 amperes is passed through a cell containing In(NO3)3 for 5.75 hours. How…

A: Faraday law of electrolysis :- In accordance with Faraday law of electrolysis mass deposited or…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 18…

Q: 4. A solution containing 0.25M copper phosphate solution containing a 2.0M H ions were subjected to…

A: Given the molarity of aqueous copper phosphate, Cu3(PO4)2 = 0.25 M Each Cu3(PO4)2 has 3 Cu2+(aq)…

Q: 7:19 AM Tue Nov 7 1 4 What is Sº for A in the reaction 3 A → 2 Bif AS°(rxn) =-132.9 J/mol K? [S° (B)…

Q: Can you explain the answer below?

A: In this question, you want to determine the atoms of Ni which are deposited on the cathode…

Q: 36) What is AG" at 25°C for the reaction (not balanced): C3H8+O2(g)-CO2(g) + H2001) if the standard…

A: We know ,∆Go = - nFE0cell Where n = number of electrons involved F = Faraday of electricity…

Q: For an electrolytic cell operating under standard conditions, if E°CELL = -0.77 V, an outside energy…

A: For an electrolytic cell operating under standard conditionsif E°cell = - 0.77V , an outside energy…

Q: Cu + Cu+ 2e 2 H,0 + 2e H2+ 2OH Calculate the amperage of the current in a cell if 1.50 g of copper…

A: By Faraday's law: w = Z.I.t w = E.I.tF 1.50 = 63.55×I×30 ×602×96500 I = 2.53 A 2.53 ampere current…

Q: None

A: Step 1: Step 2: Step 3: Step 4:

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 seconds are required to deposit 0.209 grams of cobalt metal from a solution that contains…

A: To calculate the time required to deposit 0.209 grams of cobalt metal from a solution containing…

Q: The Nernst equation can be written as E = E° In Q, what is the value | of n for the following cell?…

A: Nernst equation is used for determination of EMF of cell E=E° -RTnFlnQ where n is the number of…

Q: The electrolysis of molten AIClz for 4.25 hr with an electrical current of 25.0 A produces g of…

A: The amount of Aluminum produced can be calculated as follows

Q: Macmillan Learning Calculate the cell potential for the galvanic cell in which the given reaction…

Q: At 298 K temperature, a voltaic cell produces a standard; E°cell = 0.718 V. Calculate the value of n…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: e current in am

Q: What volumes of H2₂(9) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given process: electrolysis of watercurrent = I = 2.64 ATime = t = 15.5 minCondition : STPVolume of…

Q: What is the efficiency of a PEM hydrogen fuel cell in % if the operating voltage is 0.75V? The cell…

A: The concept used here is from Electrochemistry of physical chemistry. According to question. We…

Q: A mixture of nitric and sulfuric acids generates the nitronium ion, + NO2 (mechanism provided, which…

Q: If a water electrolysis cell operates at a current of 7.9 AA , how long will it take to generate…

Q: At the beginning (to), [Ca²+] = 0.01M, [H*] = 1M, [Hfo²+] = 2M. Consider the half-reactions below:…

A: #(d): In order to find Q value, we have to write the complete balanced equation. Since HfO2+(aq)…

Q: An electrochemical cell is based on these two half-reactions and their given standard reduction…

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

A: At STP, (which is standard temperature and pressure condition) volume is directly proportional to…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 18…

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

Heview Constants Periodie
Part A
If a water electrolysis cell operates at a current of 7.9 A, how long will it take to generate 27.0 L of hydrogen gas at a pressure of 23.0 atm and a temperature of
24 C?
R= 0.08206 Latm mol K
t- 6.78
hr
Submit
Previeus Answern Reauest Anwer

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 3 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

ellus_engine.html?ClassID=1907336612# dent Orie... One type of iron nail is coated with another metal in order to reduce corrosion. A solution of the metal, M(NO3)2 has a current of 20.00 A applied for 15.0 minutes. How many moles of M are formed during the electrolysis? [?] mol M Round only at the end. Use appropriate significant figures. Enter
What current in ampere will be required to produce 2.369 x10-3 kg of cu from CuS04 solution in one hour? (Molar mass of Cu = 63.5g/mole) Tuno vour Answer bere
A certain half-reaction has a standard reduction potential E=+0.21 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.30 V of electrical power. The cell will operate under standard conditions. l Data Note for advanced students: assume the engineer requires this half-reaction to happen at t Half-Reaction E° (V) Ag+ (aq) + e + Ag (s) A13+ (aq) + 3e - Al (s) Au+ (aq) + e - Au (s) Au3+ (aq) + 3e - Au (s) 0.7996 -1.676 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is a minimum. E = Ov 1.692 1.498 If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Ba2+ (aq) + 2e- - Ba (s) -2.912 O no minimum Br2 (1) + 2e - 2Br (aq) 1.066 Ca2+ (aq) + 2e-- Ca (s) -2.868 Cl2 (g) + 2e - 2CI (aq) Co2+ (aq) + 2e-- Co (s) Co3+ (aq) + e - Co2+ (aq) Cr2+ (aq) + 2e → Cr (s) Cr3+ (aq) + 3e +…
Please send me the question in 30 minutes it's very urgent plz
Part A If a water electrolysis cell operates at a current of 8.2 A , how long will it take to generate 23.0 L of hydrogen gas at a pressure of 27.0 atm and a temperature of 23 °C? R= 0.08206L atm mol1 K-1 t = hr
Cell Potential For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode: Ecell Ered (cathode) - Ed (anode) ▼ Tarnish on copper is the compound CuO. A tarnished copper plate i placed in an aluminum pan of boiling water. When enough salt is added so that the solution conducts electricity, the tarnish disappears. Imagine that the two halves of this redox reaction were separated and connected with a wire and a salt bridge. Part A Calculate the standard cell potential given the following standard reduction potentials: A²+ +3e Cu²+ + 20 Express your answer to two decimal places and include the appropriate units. ▸ View Available Hint(s) Ecell = li Value 4 → Units ? Al; E Cu; E 19 of 42 -1.66 V 0.340 V Review | Constants | Periodic Table
How many millimoles of O₂ (g) is produced in the anode if water is electrolyzed for 125 seconds under a constant current of 5.25 Amperes? Write answer in 3 significant figures. Do not write "millimoles" anymore, Example of answer: 0.243 for 0.243 mmol O₂. Use Faraday's constant, F = 96485 units. E° 2H₂O(1)/H2(g), 20H (aq) -0.83 V E° 2H* (aq)/H₂(g) 0.00 V Eº O2(g), 4H* (aq)/H₂O(1) 1.23 V
5a
How many seconds are required to deposit 0.150 grams of tin metal from a solution that contains Sn2+ ions, if a current of 0.652 A is applied? s