Determine the mass of Sodium (Na) produced when a 644 amp current flows for 15 hr through a cell containing molten sodium chloride (NaCI). Answer:

Q: A concentration cell is constructed of silver electrodes at 25 °C, and the half cells contain…

A: The concentration cell produces electricity due to the migration of matter from the higher…

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

A: The number of moles of a substance is determined as the mass of that substance upon its molar mass.

Q: experiment, use the experimental standard cell potential, the experimental nonstandard cell…

A: Given E°cell = 1.10 V Ecell = 1.08 V [Zn2+] = 0.10 M n = number of electrons transferred =2 Net cell…

Q: The weight of oxygen that can be generated at the anode using 800 mA after 10 minutes is: (1 Faraday…

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Q: Determine the mass of nickel that shall be electroplated from a solution of nickel (II) chloride by…

A: Given  Current (i) = 0.25 amperes Time (t) = 10 hours  = (10×60×60) seconds  t = 36000 seconds  Mass…

Q: An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.7 ampere current. What…

A: The chemical change of a substance can be accomplished by the application of an external electric…

Q: this setup: Anode Cathode electrodes Carbon Carbon solution 1.0 M CUSO4 time 20.00 minutes If 1.24…

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Q: A constant direct current was passed through a solution of copper sulfate, CuSO4, for 1 h, and 0.040…

A: A constant direct current was passed through a solution of copper sulfate, CuSO4, for 1 h, and 0.040…

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

A:

Q: The electric field strength between the plates of a simple air capacitor is equal to the voltage…

A: Given -  Voltage across the plates = 64.6 V               Electric field strength between two plates…

Q: A tub of water containing Cr³⁺(aq) is subjected to a current of 1.0 amperes for 60 minutes. How many…

A: An external source of voltage is used to carry out a reaction in case of electrochemical cell. The…

Q: A digital watch battery draws 0.20 milliamperes of current, which is provided by a mercury battery…

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Q: na cV experiment, what happens after linearly ramping to the 'switching" potential? O The potential…

A: A Cyclic Voltammetry (CV) experiment involves the scan of a range of potential voltages while…

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

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Q: How many grams of X (MW = 98.82 g/mol)(in g) will be deposited on a cathode in 2.73 h by a current…

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Q: Solving time of the electrolytic process. How long will it take for 1.25 L of a 1.0 M CuSO4 solution…

A: It is given that 1.25 L of a 1.0 M solution of CuSO4 is electrolysed under a current of 3.4 A to…

Q: The disproportionation of MnO2 (s) to Mn²+ (aq) and MnO, (aq) in acid solution at 25 °C [The…

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Q: Open Switch Closed Switch Voltage Source Voltage Source Anode Cathode, Na*) CI (Na Na Na Na Na Nat…

A: Concept of Electrolysis: Electrolysis is the passing of a direct electric current through an…

Q: grams

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Q: Calculate the reserve capacity at 80°F of an automobile battery that was discharged at 87°F for 102…

A: Reserve Capacity is the battery's capacity to keep a vehicle running if the charging mechanism…

Q: Determine the mass of Sodium (Na) produced when a 295 amp current flows for 8 hr through a cell…

A:

Q: What is the initial cell potential? Express your answer using two decimal places. HA ? Ecell =…

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

Q: Given the potential difference between the terminals of a battery as 5 Volts, calculate the number…

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Q: How many grams of silver can be plated onto an object in 5.70 minutes at 7.17 A of current? Ag*(aq)…

A: The amount of Silver plated is given below

Q: How long (in minutes) should a current of 6 amperes be applied through a solution of silver nitrate…

A: It is an application of Faraday  first law of electrolysis

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a…

A:

Q: Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction: Cu²+ (aq) +…

A: Half cell reaction :  Cu2+(aq) + 2e-   ---> Cu(s)  Mass of copper = 332 mg  Current = 6.7 A  Time…

Q: A baby’s spoon with an area of 6.25 square centimeter is plated with silver from silver  nitrate…

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

Q: Determining electrolytic activity in a dilute solution. Electrolysis of dilute aqueous NaCl solution…

A: Given: Current passed, i=10 mA=10×10-3 A

Q: If you have the reaction Fe3+ + 3e- -> Fe, how many grams of Fe will result if you apply a current…

A: Faradays first  law of electrolysis , the amount of substance  deposited at cathode   is directly…

Q: Suppose a current of 0.800 A flows through a copper wire for 22.0 minutes. Calculate how many moles…

A: Given: a current of 0.800 A flows through a copper wire for 22.0 minutes. To find: no. of moles of…

Q: A "dead" 12-Volt lead/acid storage battery has 11.30 g of PbSO4 (molar mass = 303.3 g), deposited on…

A: Answer: This question is based on Faraday's first law of electrolysis which suggests that 1 mole…

Q: Suppose a current of 520. mA flows through a copper wire for 27.0 minutes Calculate how many moles…

A: Given information: Time (t) = 27.0 minutes Current (I) = 520 mA

Q: Part C With a power supply able to produce 125 A of current, how long must the nails stay in the…

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Q: hromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If a…

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Q: What mass of gold can be plated onto an object in 7.29 minutes at 6.39 A of current? Au3+(aq) + 3e-…

A: The amount of gold plated is given below

Q: Determine the mass of Sodium( Na) produced when a 10 amp current flows for 4 hr through a cell…

A:

Q: The electrolysis of magnesium chloride can be used to produce elemental magnesium. MgCl2(l) → Mg(l)…

A: Given Chemical Reaction :: MgCl2(l) → Mg(l) + Cl2(g) Mass of Mg = ?

Q: Suppose 550.mmol of electrons must be transported from one side of an electrochemical cell to…

A: The quantity of electric charge that flows through the given solution or electrical wire is equal to…

Q: Magnesium metal is to be produced from the electrolysis of molten magnesium bromide. MgBr½(1) →…

A: Electrolysis of MgBr2 whose amount of Mg produced is to be determined.

Q: PSQ-4: A spoon is to be electroplated with Au(s) using a solution containing Au* ions. If 29.55…

A: Coulomb (C) = Ampere (A) x Second (sec) 96480 Coulomb = 1 mol e- Given: Time = 2 hours = (2 ×…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.78 minutes for a current…

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Q: How many grams of zinc, Zn(s) are electroplated out of a solution containing Zn2+ (ag) if the…

A:

Q: A 1.5 volt D-cell battery can provide a total energy equal to 40000 J. If a current of I = 1.10 A…

A:

Q: How many grams of silver can be plated onto an object in 11.37 minutes at 5.33 A of current? Ag*(aq)…

A: GivenAg+(aq.)   +  e-  →  Ag(s)Time = t = 11.37 minutes t = 11.37 min * 60 smin = 682.2 sCurrent = I…

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: The balanced reaction taking place is given as, Given: Voltage = 10 V Current = 6.0 A And mass of…

Q: A “dead” 12-Volt lead/acid storage battery has 13.00 g of PbSO4 (molar mass = 303.3 g), deposited on…

A: According to Faraday’s first law of electrolysis,

Q: What mass of gold can be plated onto an object in 12.23 minutes at 4.38 A of current? Au3+(aq) + 3e-…

A: According to Faraday's law of electrolysis -The amount of substance deposited at the electrode is…

Q: How many minutes does it take to plate 222.3 g of chromium onto a car part using 14.27 A of current?…

A: We have 222.3 g of Cr plating, current use is 14.27 A, we have to calculate the time taken for…

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.