(a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a current of 62.7 A for a period of 81.9 min? The unbalanced chemical reaction representing this electrolysis is shown below. NaNO2(aq) + H2O(l) (arrow) NO(g) + O2(g) + NaOH(aq) _______ liters of O2(g) is generated by this electrolysis.

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

A:

Q: The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one…

A: Answer: 174.0

Q: How long will it take for a uniform current of 6.00 A to deposit 78.0 g gold (197.0 g/mol) from a…

A:

Q: To what pH should you adjust a standard hydrogen electrode toachieve an electrode potential of…

A:

Q: Let’s say that you want to plate gold metal on the outside of some heart pendants (to give to all of…

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 current strength in ampere will be  required to liberate 10 g of chlorine from  sodium chloride…

A: To solve this question, use faraday's law of electrolysis which is given as follows:- m = I×tFMZ Use…

Q: What current is required to oxidize water at an electrode to liberate 1.00 mol O2/day in the…

A: Faraday first law: Mass of  substance deposited on any electrode is directly proportional to the…

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: 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: yan ecersiz sayılacaktirl. 1. 1) If a cell generates current by itself, that is, if it operates as a…

A: Given statements are : I). If a cell generate current by itself that is if it operates as a battery,…

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

A:

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: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A:

Q: 3.4 How many grams of cadmium are deposited from an aqueous solution of cadmium sulfate CdsO4 when…

A:

Q: In the electrolysis of aqueous NaCIO, how many ters of Ciy(9) (at STP) are generated by a current of…

A: Answer: 5.15e+01 L of Cl2(g) is generated

Q: Brass, an alloy of copper and zinc, can be produced by simultaneously electroplating the two metals…

A:

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

A: Given: Current = 2.96 A Time = 33.4 min Mass of V deposited at cathode = 0.784 g Molar mass of V =…

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

A: Given : Current = 50.0 A Moles of Cu formed = 5.00 mol And the ions of Cu present in the solution is…

Q: Brass, an alloy of copper and zinc, can be produced by si-multaneously electroplating the two metals…

A:

Q: Determine the current (in A) to produce 4.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A:

Q: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

A:

Q: To construct the galvanic cell illustrated above, the salt bridge was prepared by soaking a piece of…

A: Answer = The correct option is (D) According to the question - Galvanic cell -  Galvanic cell is a…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: Answer = 0.530 grams

Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

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

A:

Q: 2) How long, in minutes, will it take to plate out 25.0g of Au from a AuCl3 solution if the current…

A:

Q: = +0.851Vwhat is the spontaneous reaction between these two half-cells and what is the poten

A: For Spontaneous reaction, E°cell is positive.  Electrode with higher standard reduction potential…

Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A:

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A:

Q: A current of 3.27 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

A:

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

A:

Q: (a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a…

A: The reaction taking place is given as, => Na2O2 (aq) + H2O (l) ↔ H2 (g) + O2 (g) + NaOH (aq)…

Q: 2. In another experiment, Fischl used chromium metal to form an electrode she can use for her…

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

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: 2. In another experiment, Fischl used cadmium metal to form an electrode she can use for her voitaic…

A:

Q: What mass of each of the following duced in 1.0 h with a current of 15 A? a. Co from aqueous Co2+ b.…

A: Explained as follows

Q: An antique automobile bumper is to be chrome plated. The bumper, which is dipped into a dichromate…

A: Current passed = 21.4 A Mass of chromium to be deposited = 1.72 x 102 g Time required is to be…

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

A:

Q: Cell 1 Cell 2 Two identical spoons were electroplated with Ag or Cd through the use of the…

A: given - electroplating diagram for Ag and Cd

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: Given values:I = 0.912 ATime = 18.5 h It is known that 1 h = 3600 sec.Therefore, 18.5 h = 18.5×3600…

Q: How long will it take to plate out 4.9 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A: Given:: Mass of Ni= 4.9 g molar mass of Ni=58.6934 g mol-1 charge = ?

Q: (a) In the electrolysis of aqueous Naz2C204, how many liters of H2(9) (at STP) are generated by a…

A: The balanced chemical reaction can be written as follows: Na2C2O4 (aq) +  2H2O (l)  →  2CO2 (g) + H2…

Q: A current was passed for 5 hours through two electrolytic cells connected in series. The first cell…

A: Chemical equations for the reduction of gold and copper ions are: Au3+(aq)+3e-→Au(s)…

Q: Assuming a 5M concentration of H2SO4, and a fully dissociated electrolyte, what is the voltage of…

A: A numerical problem based on electrochemical cells that is to be accomplished.

Q: How long will it take to plate out 4.2 g Ni from aqueous Ni2+ with a current of 112.3 A? HOW DO WE…

A:

Q: When a suspected drunk driver blows 182 ml. of his breath through the fuel cell breathalyzer, the…

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.