+5 +1 +7 +1.82 V BrO3 +1.59 V +1.49 V BrO4 HBRO -1 Br | +1.07 V Br,

Q: Balance the following reaction under acidic conditions and calculate cell potential at 298K Cr2O72-…

A: Calculate  cell potential Using  Nerenst  equation

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

A:

Q: A galvanic cell is constructed in which the overall reactionis Cr,0; (aq) + 14 H2O* (aq) + 6I¯ (aq)…

A: Answer:- This question is answered by using the simple concept of calculation standard cell…

Q: If the potential of a cell is 0.51 V at 25°C when [Zn2+(aq)]=0.111M and the pressure of the hydrogen…

A:

Q: For the following redox couple, the standard reduction potential (Eed) is 1.92 V. 4+ Sn**+2e Sn+…

A: The tendency for a chemical species to get reduced and is measured in terms of volts at standard…

Q: Given the hypothetical metal samples a, B, and y were placed in an electrochemical cell as…

A: Given:  Standard reduction potential of Y = -2.38 V  E°SRP is determined by trial 1 as it contains Y…

Q: The following reduction potentials are measured at pH 0: BrO, + 6 H,O* + 5 e →B12 (e) + 9 H20 E° =…

A: The E0cell of the reaction is calculated as follows:

Q: The reaction in the Daniell cell is Cu2+ + Zn → Cu + Zn2+. (a) Given the following standard…

A: Standard potential of cell is defined as potential at 1atm and temperature of 25°c.  Note--- the…

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

A:

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

A: We have to calculate the time taken.

Q: When current is allowed to flow, which species is reduceď?

A: Species having highest reduction potential undergoes reduction at cathode.

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

A:

Q: The following cell was used for the determination of pCrO4: SCE||CrO,-(xM),Ag,CrO,(sat'd)|Ag…

A:

Q: Calculate the amounts of Cu and Br: produced at the inert elecuvues by passing a current of 4.5 A…

A: Given: Current = 4.5 A The atomic weight of Cu =63.55 gThe atomic weight of Br2=159.8 gCharge of 1…

Q: Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of…

A:

Q: Molten ScCl3 can be electrolyzed to form metallic Sc For what duratiom should an electrolysis be…

A: Molten ScCl3 can be electrolyzed to form metallic Sc. Sc3+ + 3e- -------> Sc  Given, mass of Sc =…

Q: ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited…

A: Let voltage required is V volt . And we are given 91%effeicient current = 6.82 ,so nett effective…

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

A:

Q: The cell SCE // Ag2CrO4 (sat'd), CrO42- (x M) / Ag is used for the determination of pCrO4. Calculate…

A: For the cell SCE // Ag2CrO4 (sat'd), CrO42-/ Ag, the reduction equation for silver chromate…

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

A:

Q: Calculate the minimum voltage in volts required to drive the electrolysis reaction of molten LiCl by…

A: The half-cell reactions are: Anode: Li(s) -----> Li+ + e- Eº = -3.03V Cathode: Cl2 + 2e-…

Q: Calculate the time required to precipitate 200 milligrams of copper by electrolysis of an acidic…

A: By 1F of charge 1 equivalent of metal can be deposited .

Q: The standard electrode potentials for the reduction of N2 to N2H4 and of O2 to H2O at 298 K are…

A: The EMF of an electrochemical cell is calculated by the formula: Ecello = ECo - EAo......(1) Where,…

Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E"…

A:

Q: How many liters of O2 at 298 K and 1.00 bar are produced in 2.50 hr in an electrolytic cell…

A: According to Faraday’s first law, the chemical deposition which takes place during electrolysis is…

Q: How many liters of O2 at 298 K and 1.00 bar are produced in 2.75 hr in an electrolytic cell…

A: given: Pressure (P) = 1.00 bar temperature (T) = 298 K Time (t) = 2.75 hour x 3600 = 9900 sec…

Q: Calculate the cell potential for the galvanic cell in which the reaction   Al(s)+Au3+(aq)↽−−⇀…

A:

Q: Consider this galvanic cell at 298 K:                 2 Cr(s)  +  3 Ni2+(aq)      2 Cr3+(aq)  +…

A:

Q: 1. (a) K₂Cr2O7 reacts with Fe(II) to produce Cr(III) and Fe(III) in acid medium. Write down the…

A: Reduction potential for Chromium system is 1.33 V and for iron it is 0.77 V. So, Cr2O72- will…

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

A: Faradays first law of electrolysis :- The amount of the substance deposited at the electrodes is…

Q: Determining molar mass by electrolysis. An electrolysis cell containing MSO4 solution is operated…

A:

Q: The standard reduction potential (E°) for the conversion of Cr,0 to Cr* at 25°C in an aqueous…

A: Cr2O7 2- + 14H+ + 6e- ------------------> 2Cr3+  + 7H2O            E0(Cr6+/Cr3+)   = 1.33 V  +6…

Q: Potentiometric methods of analysis are based upon measurements of the potential of electrochemical…

A: The potentiometry technique involves the measurement of cell potentials under conditions of no…

Q: Given the hypothetical metal samples a, B, and y were placed in an electrochemical cell as…

A: Answer: Standard cell potential can always be calculated using standard half cell reduction…

Q: What mass of Ni²* is produced in solution by passing a current of 67.0 A for a period of 14.0h,…

A: In the given question we have to calculate the mass of Ni2+ ion.  the given data are, Time = 14.0…

Q: A Zn Zn2 + Co 2+ Co  galvanic cell is constructed in which the standard cell potential is 0.48 V.…

A: Given: A galvanic cell :                    ZnZn2+Co2+Co                  E0cell = 0.48V = 0.48 JC-1…

Q: Compute the half-cell potential for reduction of aqueous hydronium ions to hydrogen gas at 1.3 bar…

A: The question is based on the concept of electrochemistry. we have been given hydrogen cell..we need…

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

A:

Q: A galvanic cell is constructed in which the overall reac- tion is Cr,O (aq) + 14 H,0 (aq) + 61 (aq)…

A: GALVANIC CELL A galvanic cell is an electrochemical cell that converts chemical energy into…

Q: The following cell was used for the determination of pCrO4:                     SCE||CrO42- (xM),…

A:

Q: How many liters of O2 at 298 K and 1.00 bar are produced in 1.25 hr in an electrolytic cell…

A: According to Faraday’s first law, the mass of the substance (m) deposited or liberated at any…

Q: An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of 3.00 A passing…

A: Given Current (I) = 3A Given mass = 1.572g Time = 25min = 1500s Molecular weight = 101.07g

Q: What mass of Molybdenum (Mo) could be deposited by electrolysis of an aqueous solution of Mo2(SO4)3…

A: Molar mass of Mo=95.95g/mol Provided current (i)=12.0A Provided time=125minutes Or,…

Q: How long will it take to deposit 0.0047 mol of gold by electrolysis of KAuCl4 using a constant…

A:

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given data are as follows: Cell potential =- 0.201 V Temperature = 298 K Pressure = 1 atm.

Q: Molten ScCl, can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

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.