A solution containing a metal ion (M+2, aq) is electrolyzed by a current of 7.8 A.  After 15.5 minutes , 2.39 grams of the metal is plated out.  How many coulombs are supplied by the battery?

Q: An unknown metal M forms a soluble compound, M(NO3)3. A solution of M(NO3)3 is electrolyzed. When a…

A: The deposition is M+3 (aq) + 3e– ------> M (s)Number of moles of electrons = 3 × number of moles…

Q: Suppose a galvanic cell is established using the following cell reaction, Cu(s) + 2Ag+(0.100 M)…

A: Given, The cell reaction is: Cu(s) + 2Ag+(aq)(0.100 M) <-----> Cu2+(aq) (0.200 M) + 2Ag(s)…

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A:

Q: A constant current of 1.6 A is used to precipitate copper at the cathode and oxygen at the anode of…

A: value of constant current = 1.6 A Time = 30.4 minutes cathode - copper Anode - oxygen

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

A:

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: This galvanic cell uses the reaction: Zn(s) + 2 Ag*(aq) 2 Ag(s) + Zn2+(aq) The initial…

A: The cell reaction given is, => Zn (s) + 2 Ag+ (aq) -------> 2 Ag (s) + Zn2+ (aq) Given :…

Q: A digital watch battery draws 0.40 milliamperes of current, which is provided by a mercury battery…

A: Faraday electricity: A movement of electrons is what electricity is. Relation between a number of…

Q: how many hours will the watch continue to run?

A: A device that is used to store the chemical energy and also there conversion takes place to…

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 9.8 amperes passes…

A: According to the electrochemistry Mass of substance deposited,  W = ZCt Where,   t = time in second…

Q: How many grams of silver will be obtained when the aqueous silver nitrate solution is electrolyzed…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 1.04 minutes for a current of 1.22 A to plate…

A:

Q: According to the reaction, Ag+ (aq) + e- --> Ag(s), silver is deposited. For 30.0 minutes, a 0.800A…

A:

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

A:

Q: A voltaic cell consists of a silver electrode in contact with 325 mL of 0.100 M AgNO3 solution and a…

A: Solution -

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A: To determine which electrode will be positive and the voltage that the voltmeter will show, we need…

Q: How long will an electrolytic cell containing a solution of cadmium(II) iodide need to run at a…

A:

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: A current of 5.83 A is passed through a Fe(NO3)2 solution for 1.60 h. How much iron is plated out of…

A: According to Faraday's law of electrolysis, the amount of substance deposited on an electrode is…

Q: Find the voltage of the cell if the left half cell contains 0.200 M Fe(NO₃)₂ (aq) and the right half…

A:

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

A: 1 F = 96500 C  Moles of chlorine = 1090 / 71 = 15.35 moles  Total charge = 2 × 15.35  F = 2 × 15.35…

Q: A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A: Charge flowing per unit time is known as current which may be expressed mathematically as :…

Q: A digital watch battery draws 0.35 milliamperes of current, which is provided by a mercury battery…

A: Moles of HgO and Zn is calculated as shown,

Q: ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce…

A: Use the first law of Faraday.

Q: 14.106 A voltaic cell is constructed in which the following reaction takes place: Cu (s) + 2Ag+ (aq)…

A: Number of moles of a substance is defined as ratio of mass in gram of substance to the molar mass of…

Q: A certain metal M forms a soluble sulfate salt M2SO4 . Suppose the left half cell of a galvanic cell…

A: Answer:When solution of same electrolyte with different concentrations is used in each compartment…

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

A: Number of moles = given mass / molar mass

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

A:

Q: What is the theoretical yield if this reaction initiates with 0.60 grams of acetic acid and 0.74 g…

A:

Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

A:

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

A: Mass can be calculated as:-

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 1.29 minutes for a current of 1.48 A to plate…

A:

Q: A voltaic cell is constructed at 25 °C from a half-cell in which a nickel rod is dipped into a…

A: Electrochemical cell is a cell in which chemical energy is converted to electrical energy. It is…

Q: 05 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

A: Dear student I have given answer to your question in the image format.

Q: A current of 4.05 A is passed through a Cu(NO3)2 solution for 1.70 h. How much copper is plated out…

A:

Q: Chromium can be plated from solution of CrCl3(aq) according to the following half reaction. How many…

A:

Q: A galvanic cell has the overall reaction:   2Cu+(aq) + Pb(s) → 2Cu(s) + Pb2+(aq) Which is the half…

A:

Q: (a) A student is required to construct a battery in the form of a galvanic cell using nickel (II)…

A:

Q: An unknown metal M is electrolyzed. It took 95.5 seconds for a current of 1.60 amp (A) to plate out…

A: Time taken t = 95.5 s Current I = 1.60 A Mass of metal deposited m = 0.175 g  We need to find molar…

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: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A: Given,  Concentration of left galvanic cell =1.50 M  Concentration of right galvanic cell = 75 mM

Q: You pass a 2.5 amp current through an aqueous solution of aluminum nitrate for 5 hours. How many…

A: Aluminium nitrate Al(NO3)3 has Al3+ ions Al3+ + 3 e-  -----> Al So to reduce 1 mole Al3+ ions to…

Q: A certain metal M2(SO4)3 forms a soluble sulfate salt . Suppose the left half cell of a galvanic…

A: Answer:-This question is answered by using the simple concept of electrochemistry in which…

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.