Using a current of 4.75 A, how many minutes does it take to plate onto a sculpture 1.50 grams of Cu from Copper (II) sulfate? Cu+2  +  2e-  ->  Cu Molar mass of Cu = 63.5 g/mol a. 8.0 mins b. 16.0 mins c. 958.0 mins d. 54.0 mins

Q: 1.Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which each of the…

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

Q: Calculate the voltage of the cell you would expect to measure using your Hg st

A: The cells in which  chemical energy is converted into electrical enrgy is called Gallvanic cells…

Q: Given the following half-cell reactions: Cr^+3  +  3e^-  ->  Cr           E° = -0.74 V Zn^+2  +…

A: In galvanic cell redox  reaction occur across the electrode  Here we are required to find what is…

Q: Hi there. I do not understand where I am going wrong. Any help is aappreciated!! Thanks!!   Given…

A: Given,Amount of current = 1 ampTime = 1 hourRequired,                  The solution that would…

Q: None

A: First, you need to find the molar mass of manganese. The molar mass of manganese (Mn) is…

Q: 11. What is E˚ for the following balanced reaction?   a. –0.889 V b. +1.274 V c. +0.637 V d.…

A: The electrochemical cell that utilized energy released from spontaneous chemical reaction to produce…

Q: How long will it take to plate out each of the following with a current of 200.0 Ampere? a. 1.0 kg…

A: The given current, I = 200.0 Ampere. Known, I = Qt Here, I = The current in Ampere.          t = The…

Q: 31 A current of 3.8 A is passed through a solution of AgNO3 to electroplate it onto a surface.…

A:

Q: 6. i ii Consider the following half reactions: Write the balanced half-reaction for the oxidation…

A:

Q: A baby's spoon with a surface area of 6.25 cm² is plated with silver from AgNO3 using a current 2 A…

A: Given : Surface are of spoon = 6.25 cm2  Current = 2 A And time = 2 hr 25 min = 145 mins…

Q: 20. Refer to the galvanic cell below (the contents of each half-cell are written beneath each…

A:

Q: + Cu 24 Cu Zn 2+ Zn Based on your data write a CER to answer the question: Does the potential of our…

A: Standard potentials - Cu2+ 2e---> Cu ,E°= +0.30 V Zn2+ 2e --->Zn ,E°= -0.70 V   Positive half…

Q: 2. Use standard reduction table on page 1 to help you answer this question. Cu Metal M Salt bridge…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: 7. An electrochemical cell is constructed with a tin electrode immersed in a 1.0 M SnCl2 solution…

A: standard potential of Galvanic cell = reduction potential at cathode - reduction potential at…

Q: All WOTK men A solution of NaCl (aq) is electrolyzed for 15.5 min using a current of 3.45 A. Write…

A: Given that, a solution of NaCl (aq) is electrolyzed. The time is t = 15.5 min = (15.5×60) sec = 930…

Q: 2Br + 2K* → Br₂ + 2K MM of K-39.10 g/mol MM of Br₂159.8 g/mol R=8.314 J/mol-K F-96,485 J/mol-V 4.77…

A: In electrolytic cell, oxidation and reduction reaction takes place simultaneously. The oxidation…

Q: 25 Determine the final balanced redox reaction of electrochemical cell in an experiment: a. b. C. d.…

A: Anode - Electrode where oxidation takes place Cathode - Electrode where reduction takes place

Q: 2. A spoon with an area of4.00 cm² is plated with silver from an Ag(CN),¯ solution, using a current…

A:

Q: 12. A Zinc and Copper half cell were connected under standard conditions. Calculate the standard…

A:

Q: 1. A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb²+ half-cell. a. Write balanced…

A:

Q: 9) What is the standard cell potential of a Mg and Ag electrochemical cell? (The reaction is…

A:

Q: A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag*…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: MISSED THIS? Watch KCV: Cell Potential and Concentration ; Read Section 20.6. You can click on the…

A: [Pb2+] = 0.0500 M[Cu2+] = 1.50 Mn = 2 electron transferEoCu2+/Cu = 0.34 VEoPb2+/Pb = -0.126 VEcell =…

Q: Determine the current (amps) necessary to deposit 12 grams of a metal Tr during electrolysis of Tr2+…

A:

Q: 1. If a 2.5 A current is run through a circuit for 35 minutes, how many coulombs of charge moved…

A: 1. Charge (Q) = i x t       where i = current in amperes                 t = time in seconds…

Q: Ca²+ (aq) + 2e → Ca(s) OA.0.21 V OB. -0.47 V OC -0.21 V OD.0.47 V OE. 0.42 V A Moving to another…

A:

Q: Correctly label the parts of the cell below and describe which direction the current is flowing. Mn…

A: Reduction occurs at cathode . Oxidation occurs at Anode. Current flows from cathode to anode. Salt…

Q: A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials:…

A: Galvanic cell is a type of electrochemical cell. Galvanic cell is used to supply electric current by…

Q: Consider a galvanic cell built on the following half-reactions with their standard reduction…

A: The reactions are – Oxidation half cell-2Cr3+ + 7H2O ↔Cr2O7 +14H++ 6e-.....E∘red.=1.33 VReduction…

Q: An electrochemical cell is constructed according to the line notationPt | Sn2+ (1.00 M), Sn4+ (1.00…

A: Electrochemistry is the branch of chemistry that studies the change of chemical energy into…

Q: The electrolysis of molten AICI3 for 2.50 hr with an electrical current of 12.0 A produces g of…

A:

Q: 4. A commercial cell for producing F2 operates at a current of 1500A from the electrolysis of HF…

A:

Q: A standard galvanic cell is constructed in which a Cd²* | Cd half cell acts as the cathode. Which of…

A: Given Cd2+ + 2e-  → CdECd2+/Cd0 = -0.40 VNow As the cell runs anions will migrate from Cd2+/Cd…

Q: 2. A voltaic cell is set up at 25°C with the half cells: Al3*(0.0010 M)|Al and Ni2+(0.50 M)|Ni. a.…

A: "Since there are multiple sub-parts in this question and it is not mentioned that which one has to…

Q: A cell using Zn/Zn*(aq, 1M) and. H,/H"(aq, 1M): generates a cell potential of + 0.76 V under…

A: Oxidative occurs at anode and reduction occurs at cathode. Smaller reduction potential serve as…

Q: 1. A voltaic cell is based on a Co²+ /Co half-cell and an AgC1/Ag half-cell. a. What reaction occurs…

A:

Q: Shown in the image is a diagram for the voltaic cell with the overall cell reaction being Al + Pb2+…

A: In the given cell Al electrode is anode because oxidation of Al is taking place while Pb electrode…

Q: 9. A current of 8.00 amps is passed through a molten solution of Al+3 ions for 40.0 min. How many…

A: Step 1: Step 2:Step 3: Step 4:

Q: Esmeralda the electrochemist sets up an experiment in which she plans to electroplate tin metal onto…

A: The electroplating process depends on many factors. Like electrode surface area, temperature, metal…

Q: 1.0 M CoCl, 1.0 M ZnCl, The initial voltage of the cell in the above diagram is A. 0.48 V B. -0.48 V…

A: B option is correct. Aa E= -0.48V

Q: Part A MISSED THIS? Read Section 20.6 (Pages 917-922). A Cu/Cu2+ concentration cell has a voltage of…

A: The Nernst equation is used to calculate the potential of a half-cell in an electrochemical cell, or…

Q: A voltaic cell was constructed with Au-Au³+ and Mn-Mn²+ half-cells: Given the standard reduction…

A:

Q: An rectangular metal part was coated with aluminum using a Al(NO3)3 solution. A current of 14.5 A…

A: Given,  Current, C = 14.5 A  Time, t = 56 minutes Height = 0.08 cm  Density of Al = 2.70 g/cm3

Q: How many minutes does 8.208 A of current need to be applied to plate 1.402 g of aluminum onto a…

A: Given, the half-reaction: Al3+(aq) + 3e- → Al(s) We have to find the time required that a current of…

Q: A magnesium bar with a mass of 3.2 kg is attached to a buried iron pipe to serve as a sacrificial…

A: Given: The mass of Mg bar = 3.2 Kg The current flowing through the Mg bar, (I) = 0.038 A.

Q: Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn 2+ and a silver…

A: The electrochemical cell is used to convert chemical energy to electrical energy or it may use…

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.