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

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: If the half-cell Li(s)|Li+(aq)(1.0 M) is coupled to Standard Hydrogen Electrode, will the Li(s)…

Q: Suppose a current of 680. mA flows through a copper wire for 104. seconds. Calculate how many moles…

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3906 A of…

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

Q: What mass of H₂ gas is produced during the electrolysis of water if a current of 12.7 A is used for…

A: Given, 2H+(aq) + 2e- ----> H2(g) Current (I) = 12.7 A Note: 1 min = 60 s Time (t) = 30 min = 30…

Q: An electrochemical cell is given with a cell reaction of Pb²⁺ + Cd → Pb + Cd²⁺ at 25°C with ion…

Q: A certain half-reaction has a standard reduction potential Ed=+1.14 V. An engineer proposes using…

A: The electrical power of the cell must be at least 0.60 V. the power more than this will work but…

Q: In the electrolysis of water, how long will it take to produce 1.000 × 102 L of H2 at STP (273 K and…

A: Oxidation is the process that involved the loss of electrons and oxidized to cation. Hence when a…

Q: Two identical spoons were electroplated with Ag or Cd through the use of the electrolytic cells…

A: Amount of metal deposit on spoons depends on the amount of current passed.

Q: Write the cell notation for an electrochemical cell consisting of an anode where Al (s) is oxidized…

A: Here we are required to find the cell notation for an electrochemical cell consisting of anode where…

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

Q: Which element is used to construct the standard half-cell?

A: Here given ,Multiple choice question

Q: A silver material is to be plated with gold using an aqueous solution of Au*3. How many moles of…

A: we have to calculate moles of gold deposited

Q: How many moles of O2 gas are produced at 1 atm pressure and 25 °C by the electrolysis of an aqueous…

Q: a) Nickel is immersed in 0.1M NaCl at pH = 1 and H2 pressure of 1 atm. Calculate the potential of…

A: To solve the questions regarding the electrochemical potentials involving nickel, we'll examine both…

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: Using a table of standard electrode potentials, predict whether the following reactions will be…

Q: 4+ In a standard electrochemical cell, A is reduced to solid A, while gaseous Z2 is oxidized to Z³-.…

A: Given that, A4+ is reduced to solid A, i.e., A4+(aq) → A(s). Also, gaseous Z2 is oxidized to…

Q: How many hours is required to plate 25.00g of copper metal from 1.00 M CuSO4(aq) by using a current…

A: Number of moles is calculated by dividing given mass with molecular mass. In the given question, it…

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: Calculate the number of moles of electrons driven through an electrolytic cell with 3455 A of…

A: 1- First we will determine the charge of number of electrons : We used the formula, Q = I × t…

Q: Calculate the potential (in V) resulting from an electrochemical cell if one end of a zinc wire is…

Q: Consider the following reaction: MnO4 (ag) + 5FE2+ + 8H (aq) - Mn2+ (aq) + 5FE3+ (aq) + 4H2O) (aq)…

Q: Calculate the cell potential given the standard reduction potentials for the half reactions of the…

A: The standard reduction potential for X3+ / X2+ is more than Y/Y- Therefore, reduction occur for X3+…

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

A: Faraday’s law describes that the supplied electricity deposits a definite quantity of anychemical…

Q: Calcualte the molar concentration of Ni2+ if the electrochemical cell potential has dropped to half…

A: The molar concentration of Ni2+ is to be calculated.

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

Q: In 1993 the Minnesota Department of Health set a health risk limit for 1,2-dlbromoethane In…

A: Given information, Health risk limit of 1,2-dibromoethane is 4.00 ng/L. Volume of water sample…

Q: The standard potential of zinc is E ° Zn2 + / Zn = -0.76V, while the standard reference electrode is…

A: In practice the electrical reduction potential is measured with respect to a standard electrode .…

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

A: A cell made up of the same metal and same electrolyte with different concentrations are known as…

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

Q: Calculate ΔGo, K, and Eocell indicate if the redox couple describes a galvanic or electrolytic cell…

A: A galvanic cell is one that converts chemical energy to electrical energy. It is based on a…

Q: A certain single ion channel is selectively permeable to K* and has a resistance of 1.15 G2,…

A: the answer is follows as :

Q: Calculate the cell potential given the standard reduction potentials for the half reactions of the…

A: Solution: We know at cathode reduction reaction occurs, so the half cell having highest value of…

Q: How many moles of aluminum metal would be formed by the electrolysis of Al3+ ions when a current of…

A: Given current = 8.31 Amp Time = 1.7 hour Faraday's law w =zit Where = Z = M/nF

Q: A galvanic cell is powered by the following redox reaction: 2 Cu*(aq) + H,(9) + 2OH (aq) - 2 Cu*…

Q: Assume molten ACI3 is electrolyzed with a current of 15.2 A. A3+ (aq) + 3 e¯ --> A (s) Eº = 1.04 V…

A: Faraday's law of electrolysis is given by Michael Faraday. Faraday's first law depicts that the…

Q: number of moles of electrons

Q: When [Ag*] = 1.34 M, the observed cell potential at 298K for an electrochemical cell with the…

A: Given that the concentration of Ag+ = 1.34 M the reaction is, 3 Ag+(aq)+ Al (s) → 3Ag (s) + Al3+(aq)…

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

Cd + Pb2+ <-> Cd2+ + Pb Pb: ΔHfo = ΔGfo = 0 kJ/mol. ΔSfo = 68.85 J/mol-K. Calculate the ΔG (in kJ) if the potential, E, of the cell was measured as +0.29V.
Using equation E0 = (0.0592 V / n) x log K If you choose an electrochemical reaction that transfers only one electron at a potential of 1.0 V, what would be the K? What does the value of K tell you?
F135.
What is the potential of the cell given below at 500 K? Au(s) | Au3+(0.2 M) || Au3+(0.8 M) | Au(s) 0.020 V 0.060 V 0.012 V 1.72 V 1.64 V
consider the following standard reduction potentials
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…
1. Consider the reaction: MnO2(s) + 4H*(aq)+ 2B1¯(aq) → Mn²+(aq) +Br2(1)+2H,O(1) At what pH will the voltage equal to 0 V? Considering all the other species are in standard concentrations.
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?
The electrode potential for the following two half reactions are as follows: Al+3 + 3 e- = Al(s) E = (-)1.66 V Fe+2 + 2e- = Fe(s) E = (-) 0.44 V. An electrochemical cell has an Al anode immersed in aluminum sulfate solution and a Fe cathode immersed in an iron (II) sulfate solution. The voltage generated by this cell would be: a) -2.10 V b) + 2.10 V c) -1.22 V d) + 1.22 V The number of electrons transferred in the reaction A) 2 b) 3 C0 5 d) 6
A hydrogen electrode is immersed in a 2.7 M solution of acetic acid at 25 degrees Celcius. This electrode is connected to another consisting of an iron nail dipping into 2.7 M FeCl2. What will be the measured potential of this cell? Assume Ph2=1.00