Let’s say that you want to plate gold metal on the outside of some heart pendants (to give to all of the best friends you have made online during the pandemic, of course!). You will need 0.125 g of gold in order to do this. How many minutes will it take you to plate 0.125 g of gold [from an Au(NO3)3 solution] on the pendants if you are using a current of 2.5 A?

Q: How long will it take to plate out 3.9 g Ni from aqueous Ni2+ with a current of 108.2 A? HOW DO WE…

A: To plate Ni using the process of electrolysis, the reaction that needs to be employed on the…

Q: The equilibrium constant of a cell with a cell potential of 0 V is (А) 1 B ) 2 D ) 0.5

A: The solutions are given below -

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

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

A:

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 18.0 h.If…

A: According to Faraday's first law, when a certain amount of current flows through an electrolyte, the…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by…

Q: 1. What mass of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from…

A:

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: Give an interpretation of a cell potential with a non-spontaneous reaction and a positive ΔG value

A: The relation between Gibbs free energy and Cell potential is as follows, ∆G°=-nFEcell° where, n is…

Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

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Q: The passage of a current of 0.750 A for 25.0min deposited 0.369 g of copper from a CuSO4 solution.…

A:

Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

A:

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

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Q: Manganese metal can be produced industrially by electrolysis of MnO2. How many hours would it take…

A: The compound of manganese electrolysed is MnO2 having Mn4+ ion. Hence the electrolysis reaction to…

Q: 5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4…

A:

Q: How long, in hours, must a current of 5.00 A be applied to a solution of Ag+ to produce 10.5 grams…

A: From the combination of Faraday's first and second law, we have : m = ItM/Fz  Or, t = mFz/IM ...(1)…

Q: The salt bridge in a galvanic cell allows the soltuions in the half cells to remain electrically…

A: In this question, we have to choose the correct option regarding salt bridge.

Q: Using a constant current of 7.8 A, a metal object is to be gold-plated by an electrolytic procedure…

A:

Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Since in the above reaction we can see that 1 mole of Cl2 is produced with 2 moles of electrons…

Q: A solution of NaCl is neutral, with an expected PH of 7. If electrolysis was carried out on 500 mL…

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Q: If the standard potential of a voltaic cell is + 0.831 V, what is the standard free-energy change…

A: Given standard cell potential of the Voltaic cell, Eocell = 0.831 V  Given the number of electrons…

Q: What volume of chlorine gas at standard temperature and pressure is evolved when a solution of MgCl2…

A: Provided time=1hour Molar mass of Cl2=70.906g/mol Let w gram Cl2 evolve So provided time…

Q: How many seconds are required to deposit 0.239 grams of zinc metal from a solution that contains…

A:

Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)ICr+(aq, 1.0 M) ||…

A: The cell given is, => Cr (s) | Cr3+ (aq, 1.0 M) || Ag+ (aq, 1.0 M) | Ag (s)

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: Calculate the standard cell potential of the following cell at 25°C:

A: From electrochemical cells standard reduction potential (SRP) values of Pd and Cu electrodes are…

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: Given information: Current = 12.4 A Time = 1.0 h Charge flown:  Q = It= 12.4×60×60= 44640 C For the…

Q: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

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Q: What mass of each of the following substances can be produced in 1.4 h with a current of 10. A? (a)…

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Q: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: 3. For the reaction: Zn(s) + 2Ag (aq)-Zn2(aq) 2Ag(s).. a. Determine the standard cell potential. b.…

A: Standard cell potential: E°cell =E°reduction -E°oxidation Where E°reduction = standard reduction…

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: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal calculated as follows

Q: The equilibrium constant of a cell with a cell potential of 0 V is a. 1.5 b. 2.5 c. 0 d. 1 e. 0.5 f.…

A: To Solve this problem we will calculate the equilibrium constant .

Q: 4H* + 4e + O2 -> 2 H2O, E• = + 0.82 V NAD* + H* + 2e -> NADH, E• = -0.32 V applied to the…

A:

Q: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 18 h. If 4.33…

A:

Q: A pure organic acid sample (0.1516 g) is neutralized with OH- ions produced in a constant current of…

A:

Q: 3.2 calculate the standard cell potential of the following cell at 25C 2+…

A: Standard electrode potential of equations  Cu2+ + 2e- ——> Cu(S)   Eo = 0.34V Sn2+ + 2e- ——> Sn…

Q: How long (hr) must a constant current of 50.0 A be passed through an electrolytic cell containing…

A: Answer: 5.36 hr

Q: DE What mass of each of the following substances can be duced in 1.0 h with a current of 15 A? pro-…

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

Q: How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a…

A: The mass of the substance (m) deposited or liberated at any electrode is directly proportional to…

Q: How long would it take a current of 1 ampere to reduce completely 80 cm3 of 0.10 M Fe2(SO4)3 to…

A: We can solve this problem by using the faraday law of electrolysis  W= (E×i×t)/96500 W= mass of a…

Q: How much Beryllium metal can be deposited from a solution of BeCl2 by a current of 5.0 Amperes that…

A:

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.