14.110 Which of the following statements is true regarding the electrolysis of molten NaCl? Choose the best answer. A The cathode reaction is 2CI (1)→ Cl₂ (g) + 2e- B The anode reaction is Na (1)→ Nat (1) + le¯ C CI is reduced. D Nat is oxidized. E The products are Na(1) + Cl₂ (g). Show Your Answer Check Answer Review the answer above, or select the Show Your Answer button. O O

Q: How many amperes of current needs to be passed through molten Sodium chloride to produce 2.4 g of…

A: Faraday's First law,           m α Q          m = eQ               = ect               = E96500ct…

Q: Calculate the time needed to produce 2 g of Sodium (Na) metal at the cathode when a 16 amp current…

A:

Q: Which of the following statements is true regarding a voltaic or galvanic cell? (Select all that…

A: Some of the characteristics of a voltaic or galvanic cell are : Anode is the left terminal and…

Q: 7.1 Write out a balanced half reaction for the formation of oxalate [C2O4]²- from CO2 in water.

A: Balancing of reduction reaction from CO2 to form C2O42-

Q: Current is applied to an aqueous solution of lithium bromide. What is produced at the cathode? O2(g)…

A: Oxidation occur at anode whereas reduction occur at cathode .

Q: Which statement below is not true? answer choices A) A fuel cell is a galvanic cell. B) The cell…

A: Fuel cell : It is an electrochemical cell producing energy by combining hydrogen and oxygen atoms.

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 1.8…

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

Q: QUESTION 3 Given the following cell potentials (Ecell), which would be predicted to have been found…

A:

Q: Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced…

A: The answer given earlier is absolutely correct but the mistake which is made is just a typing…

Q: In the commercial preparation of aluminum, aluminum oxide, Al2O3, is electrolyzed at 1000°C. (The…

A: Given- mass of aluminum = 3.09 kg Reaction Al3+ + 3e- ----> Al To find- coulombs of electricity…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 4.6…

A:

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: We are given two different questions.  Question 1  A setup of galvanic cell is explain and we are…

Q: 1) How many liters of cane juice is needed to supply 5g sucrose if cane juice contains 12% sucrose…

A: Since you asked multiple questions so as per Q&A guidelines of portal I solve first question…

Q: QUESTION 11 The more negative the EO value for a given reaction, the greater the tendency for the…

A: ∆E° is standard potential of a cell. For a cell ∆E° can never be negative. ∆G° = - nF∆E° That means…

Q: Which of the following species is the best oxidizing agent? Standard Reduction Potentials F₂(g) +…

A: 1)Oxidation means increase in oxidation state of the element or loss of electrons while reduction…

Q: A galvanic cell is powered by the following redox reaction: 2 Cl₂(g) + N₂H₂(aq) + 4 OH (aq) 4 Cl(aq)…

A: Given reaction is :  2Cl2 (g) + N2H4 (g) + 4OH- (aq) ------> 4Cl- (aq) + N2 (g) + 4H2O (l)  a).…

Q: 26 Consider the standard electrode potentials of the following reactions. Cr3+(aq) + 3e--Cr(s)…

A: From the value of standard reduction potential we can identify which species wil undergo reduction…

Q: Complete and balance the following redox reaction in acidic solution NO2(g) → NO3 (aq) + NO(g)

A: Balanced  chemical equation

Q: What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: At STP, (which is standard temperature and pressure condition) volume is directly proportional to…

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 9.4 amperes passes…

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

Q: Suppose 0.880 mol of electrons must be transported from one side of an electrochemical cell to…

A: Electric current is defined as the charge flown per unit time. I= Qt Where Q= Charge in coulomb t=…

Q: Calculate the time needed to produce 4.9 g of Sodium (Na) metal at the cathode when a 22 amp current…

A: Current = Charge/time I = Q/t 1Faraday = 1 F = 96500 C mol-1

Q: Electrolyzing molten MgO produces what products at the anode and cathode, respectively? A) Mg²+…

A: In an electrochemical cell, the chemical energy due to the chemical reactions is converted into…

Q: Esmeralda the electrochemist sets up an experiment in which she plans to electroplate tin metal onto…

A: Since more is the flow of electrons, more will be the production of Sn(s) as per the reaction Since…

Q: A voltaic cell is constructed with two Zn2+-Zn electrodes. The two cell compartments have [Zn2+]…

A:

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 5.1…

A: Solution: From the Faraday first law we have, the amount of chemical change being produced by a…

Q: In Electrochemical cells electrons are transfered from the reactants being reduced to the reactants…

A:

Q: What species are made at the anode and cathode, respectively, during the electrolysis of molten KBr?…

A:

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

A:

Q: Calculate the number of minutes an electroplating apparatus would have to operate at a current of…

A: time = 80.4 min

Q: Question 17 5 pts Molten sodium chloride can be electrolyzed to form liquid sodium metal and…

A: Current =15A Time= 1.25 hours=1.25 × 60 × 60 =4500seconds Temperature= 298K Pressure= 1atm Molar…

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

A: Given-> Current (I) = 1.48 ampere  Time (t) = 37.4 min = 37.5 × 60 second = 2250 seconds Weight…

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.