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

Q: com akEASSighment/takecovalentActivity.do?locator=assignment-take MISTRY [References] INTERACTIVE…

A: Here we have to calculate the time required for deposition of 1 gram of Ni from aqueous Ni^2+ with a…

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Q: Write a balanced overall reaction from these unbalanced half-reactions. Cu → Cu²+ Ag+ → Ag -

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Q: pestion 18 of 18 A current of 4.12 A is passed through a Ni(NO,), solution. How long, in hours,…

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Q: Using 1.0 A of current for 60 s, what metal solution will deposit the highest mass of metal ?…

A: NOTE : There is a typo mistake in the option. Among option a and b, one will have Fe(NO3)3. Hence…

Q: Shown below is information about a voltaic cell. Cr | Cr**(.75 M) || Ni*(?) | Niº a. Write the…

A: Expression consisting all cell's ions of any electrochemical as well as electrolytic cell is…

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: Ans is 0.546g

Q: How many seconds are required to deposit  0.207 grams of iron metal from a solution that contains…

A: According to Farady's law of electrolysis we can write m =I×t×MF×νwhereI = currentt = timeM = atomic…

Q: Given the data below: ??2?7 (??)^2− + 14 ?^+ + 6 ?^− → ??(??)^3+ + 7 ?2?(?) ?°??? = 1.33 ? ??(??)^2+…

A: Reactions are: Cr2O72− + 14H++ 6e– → 2Cr3+ + 7H2O  Ered∘=1.33V Cu2+ + 2e- → Cu  Ered∘=0.34V

Q: How many grams of chromium metal will be deposited from a solution that contains Cr3+ ions if a…

A: Faraday's 1st law of electrolysis : The amount of substance deposited is directly proportional to…

Q: How many seconds are required to deposit 0.167 grams of cadmium metal from a solution that contains…

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

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

A: The Faraday's 1st law of electrolysis is one of the most important law which explains the…

Q: Question one on the photo

A: Given information: Concentration of Cu2+ ions = 0.0010 M Temperature = 258 ℃

Q: Jaya needs to measure the unknown concentration of Sn2+. A Galvanic cell is set up in a room with a…

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Q: How many

A: Mg+2  +  2e-    -->   Mg   From Faraday's first law  W = (M / n x F)  x i x t Where W = mass of…

Q: How many seconds are required to deposit 0.268 grams of iron metal from a solution that contains…

A: Given  Mass deposited (m) = 0.268 g Current (i) = 1.22 A Time (t) = ? S The equation is Fe2+ + 2e-…

Q: at mass of

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Q: Given the cell notation below, determine the: a. Cathode and anode for the cell b. The reduction…

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

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

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Q: Investigate the formation of oxygen gas from a basic solution (formation of O2 from OH-) coupled…

A: The formation of O2 from OH- is as follows.  4OH-(aq) →O2(g) + 2H2O (l) + 4e-               ; E0Oxi…

Q: How long does it take to deposit a coating of gold 1.00 μm thick on a disk-shaped medallion 4.00 cm…

A: fist to calculate volume then to calculate mass then using formula to calculate time.

Q: What mass of Ni(s) may be deposited from an aqueous NiCl2 solution if a current of 2.50 A is applied…

A: Reaction occuring  Ni+2 (aq) + e-  --------> Ni(s)

Q: An experiment was conducted to measure the standard reduction potential, Ered of magnesium, Mg (s)…

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Q: Ağ metal is oxidized to AgCI(s) on the surface of the Ag electrode in a 0.1 M HCI solution. At a…

A: The time 1 minutes is equal to 60 second. Total number of moles of electron transferred in the…

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: How many seconds are required to deposit 0.101 grams of nickel metal from a solution that contains…

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Q: What is the current (A) required to deposit 46.0 g of Mn from a Mn²⁺(aq) solution in 1.50 hour? (F =…

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Q: 1.) The standard potential from tables for two half reactions are gven below Sn (aq) + - Sn(s) 0.136…

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

Q: Calculate the [H *] for the hydrogen half-cell of the following voltaic cell if the observed cell…

A: Here, Ecell°=1.95V. The cell is written as; Mg|Mg2+(1.00M)||H+,H2(1.00atm)|Pt

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

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Q: How many hours are required to produce 5.00 g of chromium metal from an acidic solution of potassium…

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Q: A current of 5.90 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

A: The solution is having salt Sn(NO3)2 which contains ion Sn2+  Hence on passing the current, below…

Q: Mg Mg(NO₂), Voltag ollowing statement is true 1 salt bridge contains KCI, salt bridge Ag e cell…

A: Electrolytic cell is an electrochemical device in which electric energy is converted to chemical…

Q: How many grams of  aluminum metal will be deposited from a solution that contains  Al^3+ ions if a…

A: Current = 0.826ampere Time = 55.5 minute = 55.5×60 second (1 minute = 60 second)

Q: A current of 5.739 A is applied to an unknown metal nitrate solution, M(NO3)2, for 60.0 minutes. M2+…

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Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution the…

A: Given: Time = 3.3 hours Current = 17.8 A Atomic mass of copper = 63.5 g/mol

Q: Calculate the time needed for a constant current of 0.8 A to deposit 0.1 g of a. TI(III) as the…

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Q: How long does it take to deposit a coating of gold 1.00 μm thick on a disk-shaped medallion 4.00 cm…

A: Introduction :  According to the Faraday first law of electrolysis, the amount of chemical reaction…

Q: 36 > Macmillan Learning A current of 6.00 A is passed through a Sn(NO3), solution. How long, in…

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Q: Calculate the time required for a constant current of 0.790 A to deposit 0.385 g of Tl(III) as Tl(s)…

A: Given: Current (i) = 0.790 A Mass of Tl = 0.385 g Molar mass of Tl = 204.38 g/mol

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: 23. Consider the following standard reduction potentials. E° (volts) - 2.38 Reduction Half-Reaction…

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Q: If 15.0 A of current is applied, how long would it take to produce 48 g of Cr(s)?   ___ hr

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