Part A. How many seconds are required to deposit 0.123 grams of tin metal from a solution that contains Sn2+ ions, if a current of 1.09 A is applied? ____________s   Part B. Now, how many amperes are required to deposit 0.250 grams of copper metal in 876 seconds, from a solution that contains Cu2+ ions? ____________A

Q: How many grams of gold will be plated out by a current of 0.35 A applied for 65 minutes from a…

A: Given reaction is  Au3+ (aq) +   3e-    →  Au (s) According to Faraday's law, equivalent weight of a…

Q: How many seconds are required to deposit 0.189 grams of manganese metal from a solution that…

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Q: A current of 4.76 A is passed through a Fe(NO3)2 solution for 1.20 h. Calculate the charge that…

A: Current = 4.76 A Time = 1.20 h

Q: An unknown metal M is electrolyzed. It took 672.8 s for a current of 2.50 A to plate out 0.121 g of…

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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: How many minutes are required to deposit 2.28 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

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Q: It took 2.46 min with a current of 2.03 A to plate out all the silver from 0.250 L of a solution…

A: Applying formula w=Zit

Q: Determine the molar mass (amu) of Metal (M) if it took 1.57 minutes for a current of 1.09 A to plate…

A: First we would calculate the charge using formula : Q = I × t Then we would calculate the moles of…

Q: How many minutes are required to deposit 1.39 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A:

Q: How many minutes are required to deposit 1.42 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: Given:  W = 1.42 gm  I = 2.50 A  Mol. Wt. of Cr = 52  'n' factor of Cr = 3  Equivalent wt. of Cr =…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.55 minutes for a current…

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Q: An unknown metal M is electrolyzed. It took 672.8 s for a current of 2.50 A to plate out 0.121 g of…

A: According to Faraday’s first law, the mass of the substance (m) deposited or liberated at any…

Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.4 kg is attached to a buried…

A: The solution is given below -

Q: Determine the molar mass (AMU) of Metal (M) if it took 2.56 minutes for a current of 1.11 A to plate…

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A: Ionic gold gains 3 electrons to get reduced to metallic gold Au3+ + 3e-  --> Au

Q: How long (in minutes) should a current of 5.6 amperes be applied through a solution of silver…

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Q: How many grams of zinc metal will be deposited from a solution that contains Zn2* ions if a current…

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Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

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A: a.) To calculate number of electrons , we would check the charge on gold ion . b.) To calculate…

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Q: How many minutes are required to deposit 1.48 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

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Q: 15. How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…

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A: We have given the mass of gold that has to be deposited = 55.0 g Current = I = 2.225 A MM of gold =…

Q: How many grams of Ag would be deposited from an aqueous solution of Ag+ with a current of 2.534 A…

A: Molar mass of Ag = 108g/mol Reaction takes place:- Ag+ + e-  ------> Ag  current , I = 2.534 A…

Q: A current of 3.33 A is passed through a Sn(NO3)₂ solution for 1.30 h. How much tin is plated out of…

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Q: OI Ag zed will a Coist A mtil 0.15 mols of metal is deposited. Which metal will require the greatest…

A: Current I is given as I= Q /t ,where Q is the charge flown in time t.  So t= Q/I

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A: According to electro-chemistry  W = zCt W= mass of Metal deposited in grams C= current  t = time in…

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Q: 9. How many grams of Cu are plated out from a CuSO4 solution by a current of 7.8 amps flowing for…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.12 minutes for a current…

A: Given: Time = 1.12 minutes = 1.12×60 sec Correct = 1.22 A Mass of the metal M = 0.0896 g

Q: How many amperes are required to deposit 0.177 grams of tin metal in 872 seconds, from a solution…

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Q: How many grams of zinc metal will be deposited from a solution that contains Zn² ions if a current…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.07 minutes for a current…

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Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: How many minutes are required to deposit 2.73 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: Given : I= 2.50 A F = 96500 C/mol Quantity of charged passed = I*t = 2.5*t = 2.5t 2.5t C deposits Cr…

Q: How much time is needed for a 1.00 g Ag to be deposited by electrolysis of a AgNO3 solution using a…

A: