Molten ScCl3 can be electrolyzed to form metallic Sc For what duratiom should an electrolysis be performed at a current of 1.03A in order to produce 29.3g Sc?   _______ s

Q: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous…

A: Electrical energy=0.1599 kWh

Q: Consider the reaction at 25°C (Masterton et al., 2012) Mn02(s) + 4 Hčaq) + 2 Brīag) 2+ → Mnfag) +…

A: We have been asked to find the pH at which the voltage is zero. Reaction is at 25°C

Q: Example: A steel coupon with an anode surface area of 1000 cm2 is placed in an electrolyte. The…

A: The current, I = 1 mA Or 0.001 A

Q: A corrosion cell consists of copper(Cu) with an sheet area of 250cm2 and the density of the current…

A: Given: Surface area of Cu = 250 cm2  Surface area of Fe = 25 cm2  And current density passing = 0.5…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.14 minutes for a current…

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Q: (b) A constant current was passed through a solution of AuCl; between gold (Au) electrodes. After a…

A: Given, Mass of gold deposited = 2.628g Time = 20min = 1200 second

Q: Determine the molar mass (amu) of Metal (M) if it took 2.35 minutes for a current of 1.06 A to plate…

A:

Q: Cu| Cu2+ (x M) || Cu2+ (y M) | Cu Verify the accuracy of the cell potentials measured at 27.5°C…

A: Concentration cells are the electrochemical cells that contain same electrode and electrolyte in the…

Q: A corrosion cell consists of copper(Cu) with an sheet area of 250cm2 and the density of the current…

A: Given: Surface area of Cu = 250 cm2  Surface area of Fe = 25 cm2  And current density passing = 0.5…

Q: 3. Consider the reaction at 25°C Mn02(s) + 4 Hiag) + 2 Brīag) → Mnag) + Brz) + 2H20) At what pH is…

A: To determine the Eo of the given cell, At anode:Br2(l) + 2e- →2Br-(aq) ; E° = +1.080 VAt…

Q: How many seconds are required to deposit 0.143 grams of tin metal from a solution that contains Sn2+…

A: Answer: Since, Sn2+ is getting reduced into Sn, therefore its valency factor will be 2 and its…

Q: ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited…

A: Given: Current = 6.86 A Time passed = 9 hour Power = 0.1573 KWh. Current efficiency = 80 %

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: A cylindrical metal carries a current of 10 A. What will be its diameter, in mm, if the minimum…

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Q: 1. Thirty minutes (30 m) of electrolysis of a solution of CuSO4 produced 3.75 g of Cu at the…

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

Q: otentials. 2 +2H2O + 4e --> 40H Enote = 0.401V a2+ 2e ----> Ca Enote = -2.868 alculate the maximum…

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Q: pH

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Q: (i) Define electroplating. Give any two uses of electroplating. ii) To electroplate 7.5 mg of Cu on…

A: 1. electroplating -  Electroplating is the process of plating one metal onto another by hydrolysis,…

Q: For a PEM fuel cell (n=2 and F= 96500 C/mole), if the AH is -240 kJ/mole at standard conditions, the…

A: Given  PEM fule cell ( n= 2 and f= 96500 c/ mole) H is - 240 kj/ mole  Voltage is 0.8 V  And fule…

Q: Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of…

A: Given: Surface are of the plate = 7.73 cm2  Density of copper = 8.96 g/cm3  Current passed = 4.54 A…

Q: unknown metal (M) was electrodeposited from an aqueous solution containing M2X2 (where X is the…

A:

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Given: Current = 2.96 A Time = 33.4 min Mass of V deposited at cathode = 0.784 g Molar mass of V =…

Q: e) Determine the Gibbs energy change per mole of reaction. Faraday's constant is 96485 reduction…

A: Anodic reaction:                                  C2O42-  -----------> 2CO2 + 2e- ---------(1)…

Q: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous…

A: Electrical energy=0.1145 kWh

Q: Make an inference about the effect of concentration on the cell potential. Thoroughly explain and…

A: Since you have asked multiple questions, we will answer first question for you. In order to get…

Q: A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A: Charge flowing per unit time is known as current which may be expressed mathematically as :…

Q: A steel coupon with an anode surface area of 1000 cm is placed in an electrolyte. The corrosion…

A: Electrochemical equivalent is the amount of element deposited at an electrode when one ampere of…

Q: The purity of a sample of K3Fe(CN)6 is determined using hydrodynamic voltammetry at a glassy carbon…

A: a)   Here, the similar chemical is used for calibration, but is not added to the sample to be…

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

A: Given: ScCl3 can be electrolyzed to form metallic Sc. We have to calculate the time required for the…

Q: An electrolysis cell containing MSO4 solution is operated for 1.0 h at a constant current of 0.200…

A: Given,  An electrolysis of MSO4 solution for 1.0 h at a constant current of 0.200 A. If the current…

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: Pb4+(aq) + 2e-  Pb2+(aq) ΔHfo = ΔGfo = 0 kJ/mol. ΔSfo = 68.85 J/mol-K. Calculate the cell voltage,…

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Q: Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of…

A:

Q: A current of 0.045 A rag meagund for the Lu /Zn cell prepaned In beconels, Caleulate how long it…

A: Given, Magnitude of current = 0.045 A Mass of copper deposited = 1g Molar  mass of copper = 63.646…

Q: Consider a cell whose Nernst potential is 0.50 V. If the cell resistance is 7.50 ohms and a current…

A: Overpotential is the measure of excess potential required to derive a reaction from its…

Q: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous…

A: Electrical energy consumed = 0.2018 kWh.

Q: Liquid-Junction potentials can be ignored in the calculation for the reduction potential of a cell…

A: Boundary between two electrolyte solution of different composition and across the boundary a…

Q: If the concentration of Na+ inside of a cell increases, the Nernst potential for Na+ will do what?

A:

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: Halogen lightbulb filaments are sometimes made from a high melting point metal. The most common ore…

A: Given :-  Current Passed = I = 74.00 A = 74.00 C/s Time = t = 709.2 minutes = 42552 s   Metal M…

Q: Find the electric potential (E) for the following reaction at 350K when [Al3+] = 0.27 M, and [Cr3+]…

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Q: What amount of electrons, in moles, is required to perform the electrolysis? 0.420 mol Sc desired 3…

A: Molar mass of Sc = 44.95 g/mol

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Current I = 1.46 A  time t = 23.1 minutes = 23.1 * 60 s = 1386 s Mass of vanadium deposited = 0.534…

Q: ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited…

A: Given: Current supplied, Q = 4.47 A  Time, t = 12 h Electrical energy = 0.1885 kWh Current…

Q: 6. The corrosion potential of mild steel in a deaerated solution of pH = 2 is -0.64 V versus…

A: The reactions that occur in the given cell are stated below:

Q: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous…

A: Answer: Current efficiency given is 87%, therefore actual current passed…

Q: 5. A student-produced a plot of Ecei vs. In[Cu2-] which had an equation of y = -0.0977x + 0.0057.…

A:

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.24 minutes for a current…

A: