Suppose that electrons flow into a solution containing Sn4+, which causes the following reduction reaction: Sn4++2e- → Sn2+ If the aplied current is 0.505 A, what is the rate of Sn2+ being generated? (in kg/h) a) 4.48x10-3 b)4.48 c) 2.24x10-3 d) 1.12 x 10-3 e) 0.56 x10-3

Q: salt bridge 1.0 M (aq) 1.0 M (aq) Anode Cathode 1. A student constructs a voltaic cell to study the…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: What mass of Mg is produced (in grams) when a constant current of 0.752 A is passed through an…

A: Given current (I) = 0.752 A time (t) = 14.2 hours molar mass = 24.31 g/mol electrons transfer  = 2

Q: Part A. How many seconds are required to deposit 0.123 grams of tin metal from a solution that…

A: Faraday's law in electrolysis:

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Q: E°zn2-/z0) = -0.763 V MMz = 65.38 g/mol Zn2+(aq) +2e--Zn(s) a.) If a current of 35.0 amps flows for…

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Q: A current of 3.37 A is passed through a Cu(NO3)2Cu(NO3)2 solution for 1.30 h. How much copper is…

A: Given, the current = 3.37 A Time = 1.30 hour Now change the current (From A to C/s) and time (min…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current of 1.2 A to plate…

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Q: The redox reaction below has a AG value of 219. kJ. Determine the standard cell potential (Eᵒcell)…

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Q: Calculate the mass in grams of zinc that will deposit on a metal washer if a current of 25.0 A is…

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Q: A     constant current     of     0.800     A     is     used to deposit copper     at    the…

A: I = 0.8A t = 15.2min F = 96485 C Cu deposited at cathode. O2 deposited at anode. Mol. mass of Cu =…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.02 minutes for a current…

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Q: Consider an electrolytic cell with a steady current of 158 amperes which produces Als) (atomic mass…

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Q: What mass of Mg is produced (in grams) when a constant current of 0.945 A is passed through an…

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Q: A certain half-reaction has a standard reduction potential E=-0.44 V. An engineer proposes using thH…

A: GivenEred0(anode) = -0.44 VEcell0 ≥ 1.20 V

Q: What is the voltage for the following reaction 25°C: AgIAg" (0.14M)IHg2"(0.06M)|Hg

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Q: When the Hg2+ concentration is 1.01 M, the observed cell potential at 298K for an electrochemical…

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Q: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

A: Given The amount of current (I) is 2.15 A The time is 2.2 hours The density of zinc is 7.410 g/cm3…

Q: MISSED THIS? Read Section 20.6 (Pages 917 - 922) . Part A An electrochemical cell is based on the…

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Q: How many milliliters of oxygen gas is generated from electrolysis of water performed at 25°C using a…

A: Electrolysis of watercathode: 2H++2e-→H2,       n=2anode: 40H-→O2+4e-+2H2O,   n44

Q: How long will it take for the following to plate out each of the following with a current of 100 A?…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.52 minutes for a current…

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Q: standard galvanic cell is constructed with Sn²* | Sn and Ni* | Ni half cell compartments connected…

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Q: 3. Use a table of standard thermodynamic values to predict the standard cell potential at 71 C:…

A: Given cell notation is :  Cu(s) | CuSO4 || AgNO3 | Ag (s)  Use the standard thermodynamics values to…

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A: We have to find the E cell of given reaction

Q: What current is needed in order to remove 1.00 g of nickel from Ni(NO3)4(aq) solution in 1.00 hour?…

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Q: Alkaline dry-cell batteries have a voltage of 1.50 V under standard conditions.  Given this standard…

A: Chemically, a typical alkaline dry cell battery has a zinc anode and a manganese dioxide cathode.…

Q: current

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.66 minutes for a current…

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Q: Using a current of 4.75 A, how many minutes does it take to plate onto a sculpture 1.50 grams of Cu…

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Q: 405−mL solution of NaCl was electrolyzed for 5.80 min. If the pH of the final solution was 12.23,…

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Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 119.9 A? WHERE ARE…

A: Given:: Mass of Ni = 1.0 g molar mass of Ni = 58.6934 g mol-1 Current = 119.9 A Time (t)  = ?

Q: A student deposited 2.50 g of zinc (65.39 g/mol) onto a sculpture from a ZnSO4 solution. The…

A: Given that : The mass of zinc deposited = 2.50 g Molar mass of Zn = 65.39 g/mol Current supplied =…

Q: What current (in A) is required toplate out 1.22 g of nickel from a solution of Ni2+ in 1.0…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.57 minutes for a current…

A: Using the formula for mass deposition to solve this.

Q: HTERACTIVE EXAMPLE Electroplating How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with…

A: Given :  Mass of Ni = 1.0 g  Current (I) = 119.9 A  Molar mass of Nickel = 58.7 gm/mol

Q: One type of iron nail is coated with another metal in order to reduce corrosion. A solution of the…

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Q: CHEMWORK An aqueous solution of PdCl, is electrolyzed for 90.7 seconds and during this time 0.1064 g…

A: We have given that  Mass of Pd deposited = 0.1064g  time = 90.7sec  F = 96485C/mol  i = current = ?…

Q: Example 9. In an electrolysis experiment, a current was passed for 5 hours through two cells…

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

Q: . How much Cr(s) will plate out of a K2CrO4 solution if we use a current of 15A for 1 hour?…

A: Given,  Current (i) = 15 A Time = 1 hr = 3600 s Moalr mass(M) of Cr = 52 g/mol Number of electrons…

Q: What is the oxidation number of manganese (Mn) in a sample of unknown compound when application of a…

A: According to Faraday's law of Electrolysis we can write,  m=I×t×MF×nwherem= mass of metal…

Q: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

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Q: 670.24 sec

A: Given data are as follows: Weight of silver deposited = 1.5 g Current passed = 2A

Q: The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution)…

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Q: How many millimoles of O₂ (g) is produced in the anode if water is electrolyzed for 125 seconds…

A: Given :  Time (t) = 125 seconds  Current (I) = 5.25 A  Faraday's constant, F = 96485 units

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.96 minutes for a current…

A: Metal is deposited as M3++3e-= 3M . We can infer that 3moles of electrons=3Faraday=3×96485 = 289455…

Q: A baby'sspoon with an area of 6.25 cm2 is plated with silver from AgN03 using a current of 2.00 A…

A: (a),

Q: Example 10. How long has a current of 3 ampere to be ap- plied through a solution of silver nitrate…

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Q: Given a half-reaction: 2I- → I2 + 2e-  Given: Current = 461 mA time = 3min faradays constant…

A: The Faraday’s Laws of electrolysis gives the information about the quantitative aspects taken place…

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.