What mass of calcium can be produced by this process if a current of 5700 A is applied for 53 h? Assume that the electrolytic cell is 75 % efficient. Express your answer using two significant figures. Submit ΑΣΦ Request Answer ? g Ca

What mass of calcium can be produced by this process if a current of 5700 A is applied for 53 h? Assume that the electrolytic cell is 75 % efficient. Express your answer using two significant figures. Submit ΑΣΦ Request Answer ? g Ca

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 galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu?* (aq)…

A: Since in the above reaction, Cu2+ is being reduced to Cu and Al is being oxidised to Al3+ Hence the…

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

A: Given that, a cell reaction is Cu2+aq + Zns →Cus + Zn2+aq. The concentrations are [Cu2+] = 1.16 M…

Q: A Cr/Cr3* concentration cell has a voltage of 0.083 V at 25 °C. The concentration of Cr3+ in the…

A: Answer:- This question is answered by using the simple concept of calculation of concentration using…

Q: two grams of copper (A.W. = 63.54g g/mol, density = 8.93g/cm^3) dissolves in 500g of water to…

A: Reaction: Cu→Cu2+ + 2e- Using Nernst equation: ECell=Ecell∘-0.05912logCu2+

Q: A cell contains 100 mM K+ and is surrounded by interstitial fluid containing 10 mM K+. The…

A: The objective is to determine the temperature of the cells.Given:Equilibrium potential…

Q: 18.83. Calculate the minimum (least negative) cathode potential (versus SHE) needed to begin…

A: For electroplating we need to reduce the Ni2+ to Ni on iron piece.

Q: Calculate the time needed to operate an electrolytic cell to plate 0.53 g of Z that is running at…

Q: How many grams of X (MW = 98.82 g/mol)(in g) will be deposited on a cathode in 2.73 h by a current…

Q: How many liters of O2 at 298 K and 1.00 bar are produced in 4.00 hr in an electrolytic cell…

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 aluminum can be produced by the electrolysis of an aluminum chloride solution,…

A: Calculate the moles of e-, Al3+ + 3 e- → AlCharge (C) = Current (A) × Time (s) = 15.0…

Q: Stacy has class is from 10:30 am-1:20 pm, in which she performed an electrolysis experiment with…

A: This can be proved according to the Faraday's first law of electrolysis. It states that, Mass of the…

Q: What is the cell potential when 0.1 M C u(NO3)2 and 1.0 M A l(NO3)3 are used? Answer to two decimal…

A: The given electrochemical cell consists of two half-reactions, one involving copper ions (Cu2+) and…

Q: hey wanted to produce a cell with an operating potential of 1.05 V and calculated that Q for the…

Q: when using the equation Q=It in electro chem, how do you find the Q value if not given t. Is it mols…

A: In the equation, shown in equation (1), t is defined by time duration for the current of I (in A),…

Q: Show your work with tables 1 Amp means 1 C/1 sec 5 amp means 5C per 1 sec Faraday’s…

A: Given current is 15A. Farady constant is given as 96,485 C. Time for which the current is passed…

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

A: Given data: Concentration of solution = 0.4 M Emf of cell = 0.015 V Formula used:…

Q: A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation,…

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

Q: MISSED THIS? Watch KCV 19.6; Read Section 19.6. You can click on the Review link to access the…

Q: What is the emf of this cell when [Fe2+] = 1.8 M, [Fe+] = 1.2x10-2 M , Po, = 0.55 atm , and the pH…

A: The voltaic cell reaction given is 4 Fe2+ (aq) + O2 (g) + 4 H+ (aq) → 4 Fe3+ (aq) + 2 H2O (l) The…

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

A: Given is the Nerst equation in which E° is the standard cell potential while Q is reaction quotient.…

Q: If zinc has a density of 7.14 g/cm³, (a) what mass of zinc is required to cover a plate of iron that…

A: Given, Density of zinc =7.14gcm3

Q: A voltaic cell utilizes the following reaction: 2Fe³+ (aq) + H₂(g) →2Fe²+ (aq) + 2H+ (aq). You may…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu*…

Q: Calculate the mass (in grams) of K formed by a current of 6.5 x 104 A flowing for 24 hours if the…

Q: Cd + Pb2+ Cd2+ + Pb Pb: ΔHfo = ΔGfo = 0 kJ/mol. ΔSfo = 68.85 J/mol-K. Calculate the ΔG (in kJ) if…

A: Given: Cell potential (E) of the cell = +0.29 V.

Q: For the following galvanic cell (expressed in cell notation), how will the voltage, E, change if…

A: Given cell : X | X+ || Fe 2+ | Fe Reaction at cathode: Fe 2+ + 2e --> FeReaction at anode: X…

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

Elemental calcium is produced by the electrolysis of
molten CaCl₂
What mass of calcium can be produced by this process if a current of 5700 A is applied for
53 h? Assume that the electrolytic cell is 75% efficient.
Express your answer using two significant figures.
Submit
Part B
ΑΣΦΑ
Ell-
Request Answer
?
g Ca
What is the minimum voltage needed to cause the electrolysis?
Express your answer using three significant figures.
197| ΑΣΦ
?
V

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: Introduction

Step 2: A part

Step 3: B part

Solution

Trending now

This is a popular solution!

Step by step

Solved in 4 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

Consider the following galvanic cell: E° (V) U3+ + 3 e− → U(s) −1.642 In3+ + 2e− → In+ −0.444 What is the potential of the galvanic cell when In3+ is 0.023 M, In+ is 0.37 M, and U3+ is 0.076 M?
The Nernst Equation A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT InQ nF E = E° - where E = potential under nonstandard conditions %3D E = standard potential R = ideal gas constant = 8.314 J/K mol %3D T = kelvin temperature n = number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons = %3D 96, 485 C/mol = 96, 485 J/V mol %3D Q = reaction quotient %3D It is customary to use the equation in a form where numberical values are substituted for R, T, and F at a temperature of 25°C. (8.314 J/K mol)(298K) 96, 485 J/V mol RT = 0.02568 V %3D and the Nernst equation with the potentials in volts is: 0.02568 In Q E = E - n Sometimes it is more convenient to use base-10 logarithms, and the substitution of 2.3026 log for In is made. (2.3026 x 0.02568 = 0.0591) %3D 0.0591 logQ E = E° – A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. Use…
If 21.42 mL of 0.1360 M NaOH is needed to fully titrate a solution made with 0.1422 g of a diprotic acid, what is the experimental molar mass of the acid? 75.46 g/mol 612.8 g/mol 211.7 g/mol 97.63 g/mol 553.8 g/mol
For the cell at 298 K outlined below, answer the questions. The cell volumes are 100.0 ml. Au (s) | Au3+ (0.8 M) || Ag+ (0.6 M) | Ag (s) What is DeltaG of the cell? If a current of 1.2 amps is drawn from the cell for 10800 seconds. What is Ecell at that point?
Determine concentration of an electric cell solution