An electrolytic cell contains 50.0 mL of a 0.297M solution of Fe Cl3. A current of 0.643 A is passed through the cell, causing deposition of Fe(s) at the cathode. What is the concentration of Fe* (aq) in the cell after this current has run for 15.0 min? Concentration = M

Q: Calculate the standard cell potential, Ecell°, for the reaction shown. Use these standard reduction…

A: The standard cell potentials are= For the Cu+| Cu half cell = 0.521 V For the Ag+ |Ag half cell =…

Q: A 0.100 M neutral aqueous CaCl2 solution is electrolyzed using platinum electrodes. A current of…

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Q: Silver can be electroplated at the cathode of an electrolysis cell according to the following…

A: Given information:Current (I) = 6.4 ATime (t) = 69 minutes

Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given that: Mass of chromium deposited = 14.5 g Amount of current passed through solution = 4.57 A…

Q: Copper metal can be purified electrolytically according to the following arrangement. The anode is…

A: W = I × t × M / n × F Where ; W = mass of  purified Cu = ? I = current = 15 A  t = time = 8.5 hours…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 4.65…

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Q: A galvanic cell is constructed that carries out the reaction 2Ag(s) + Cl2 (g) → 2Ag+(aq) + 2CI- (ag)…

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Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: What amount of Cu (in grams) is deposited at the cathode when a current of 6 A is maintained for 15…

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Q: An electrolytic cell consists of a pair of inert metallic electrodes in a solution buffered to pH =…

A: Part a: The electrolytic cell consists of two electrodes, anode and cathode. Oxidation occurs at…

Q: If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2 amps in an…

A: Given, If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2…

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Q: 1. Given the following reduction potentials: Ag*(aq) + e → Ag(s) Zn (aq) + 20ZN(s) Calculate the…

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

Q: b) Balance the following redox reaction in aqueous basic solution: NO3 + Fe(CN),* NO9) + Fe(CN)6…

A: Balanced the given redox reaction in aqueous basic solution---

Q: Calculate the mass of silver (Ag +1 ) deposited at the cathode during the electrolysis of silver…

A: Reduction → gain of electronReduction always occurs at CathodeAg++ e-  →Ag

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Q: Balance each redox reaction occurring in acidic aqueous solution. a. PbO,(s) + T(aq) + Pb*(aq) +…

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Q: a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

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Q: 19.69 Calculate the standard cell potential of the following cell at 25°C.…

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Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

Q: Balance each redox reaction in acid solution. H,O2 + Cr0, +02 + Teo, + N;O. → Te + NO,

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Q: An aqueous solution contains a mixture of cations at the following concentrations.…

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Q: 4. What current is required to deposit on the cathode 5.00 g gold/h from a solution containing a…

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Q: A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at…

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Q: Balance the following redox reaction in basic solution. 2+ N,H,(aq)+Zn (aq) N2(g)+Zn(s) 2+ N,H, (ag)…

A: Balanced the given redox reactio under basic condition--- N2H4(aq) + Zn2+(aq) ----> N2(g) + Zn(s)…

Q: A gold (III) chloride solution was electrolyzed using a current of 13.5 amperes for four hours. How…

A: Mass deposit or plated  = Z.i.t

Q: Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45…

A: In a electrolytic process, cations go to the anode and anions go to the cathode.

Q: Calculate the standard cell potential, E, for the reaction shown. Use these standard reduction…

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Q: grams of iron

A:

Q: Using values from the tables of standard reduction potentials, calculate the cell potential of the…

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A: Hii there, since there are multiple questions posted. We are answering first question. If you need…

Q: Balance the redox reaction below in basic solution. PbO2(s) + 1(aq) Pb2*(aq) + I2(s) How many OH…

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Q: A galvanic cell is constructed that carries out the reaction 2 Ag(s) + Cl, (g) 2 Ag* (aq) + 2 CI…

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Q: Balance each redox reaction occurring in acidic aqueous solution. a. I (aq) + NO, (aq) 1,(s) + NO(g)

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Q: b) Fe(CN),³(aq) + + Re(s) >Fe(CN),*(aq) + ReO,'(aq) [basic]

A: To Balance the reaction first we divided it into  half reduction and oxidation reaction

Q: 4. A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper (II)…

A: Anode is the electrode on which oxidation takes place and Cathode is the electrode where reduction…

Q: Balance the following redox reaction in aqueous basic solution: NO (g) + Fe(CN)6 (aq) 4- NO3 +…

A:

Q: Balance the redox reaction below in basic solution. PbO2(s) + 1'(aq) Pb2*(aq) + I2(s) How many OH…

A: Redox reaction is a reaction involving simultaneous oxidation an reduction.

Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given data:  Current = 4.57 A  Cr deposited = 14.5 g  Molar mass of Cr = 52 g.mol-  CrCl3  ==>…

Q: Use standard reduction potentials to find the equilibrium constant for the following reaction at…

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Q: What mass of gold is produced when 15.2 A of current are passed through a gold solution for 25.0 min

A: Given information: Current (I) = 15.2 A Time (t) = 25.0 min

Q: A strip of nickel metal is placed in a 1 molar solution of Ni(NO3)2 and a strip of silver metal is…

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Q: Consider the following standard reduction potentials Ag*(aq) + E→AB(s) E° = 0.80 v %3D Ag(NH3)2*(aq)…

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Q: Copper(I) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with…

A: Answer :- 1.45 × 1012  The equilibrium constant (K) at 25°C for the given reaction = 1.45 × 1012…

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.