An unknown metal, X, has been deposited on the cathode of an electrolytic cell using an electric current of 3.30 Amps for a period of 25.0 mins:  2X2+ + 2 e– → X  The mass of X collected at the cathode was 1.51 g.  Identify the unknown metal, X.

Q: A total of 1.740 F of electricity (1 F=1 mol e−) was required to electrodeposit all of the Zn and Co…

A: The mass of each compound is calculated by the number of moles of the compound. The number of moles…

Q: A total of 1.429 F of electricity (1 F = 1 mol e) was required to electrodeposit all of the Zn and…

A:

Q: Balance the following chemical reaction using the half reaction method and identify the oxidizing…

A: The Given reaction in acidic medium  HNO3(aq) + SO42-(aq) + Pb(s) → NO(g) + PbSO4(s) = [acidic]

Q: Balance the following redox reaction under basic conditions. H2O2(aq) + CIO2(aq)→ CIO2(aq) + O2(g)

A: We have to Balance the Redox Reaction in the Basic medium.

Q: Calculate the mass of silver that would be deposited by a battery that delivers 1.3 A•hr of charge.…

A: Given: Current = 1.3 Amp time = 1 hr = 3600 s   Electrochemical reaction of silver is given by,…

Q: Complete and balance the following redox reaction in basic solution. Be sure to include the proper…

A: The given redox reaction is as follows: A redox reaction is balanced by balancing the mass and…

Q: Describe the anode and cathode of an electrolytic cell in which gold is to beplated on an object.

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Q: Balance the following redox reaction in acidic solution. 2+ Zn(s) + O₂(g) Zn(aq) + H₂O(1) - 2+ Zn…

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Q: Balance the following redox reaction in acidic solution using the half reactions method. CuS (s) +…

A: Please find your solution below  :

Q: balance the reaction in acidic solution • identify the species oxidized, the species reduced, the…

A: We will give all required information.

Q: Four metals (A, B, C, and D) were studied for activity, and the following information was  collected…

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Q: What are the products in the electrolysis of aqueous copper (II) iodide?

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Q: Balance the following redox reaction under basic conditions. NiO2(s) + Si(s)→Ni(OH)2(aq) +…

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Q: Which of the following metals is most likely to become oxidized (act as O Ca2+(aq)+2e¯→ Ca(s) E°red=…

A: Introduction : Oxidation means loss of electron .

Q: Consider the voltaic cell illustrated in the figure (Figure 1), which is based on the cell reaction…

A: G = -nFE = J/mol Zn(s)-->Zn^2+(aq)+2e^- 0.765 V Cu^2+(aq)+2e^- -->Cu(s) 0.337 V   n = 2, F =…

Q: Write a balanced chemical equation (including states of matter) for an electrochemical cell that has…

A: An electrochemical cell is a device which is used to generate electrical energy from the chemical…

Q: Which metal will get oxidized? what is the total Coulomb?

A: Those metal which have high standard reduction potential act ascathode & low reduction potential…

Q: Find the emf of the concentration cell at 25.0 ºC in which the concentration of Ag+ ions in the…

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Q: A total of 1.638 F of electricity (1 F = 1 mol e) was required to electrodeposit all of the Zn and…

A:

Q: Balance the following equation for acid conditions by the half-reaction method. Identify the…

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Q: Balance the following redox reaction that occurs under basic, aqueous conditions: NiO2 + Fe →…

A: To balance a redox reaction,follow the below mentioned steps: 1) Consider oxidation and reduction…

Q: species that were reduced and oxidized. + MnO; → HCOO + MnOz CH:OH

A: Oxidation half: CH3OH   ----->  HCOO-    Reduction half: MnO4-  ------>  MnO2

Q: A total of 1.558 F of electricity (1 F = 1 mol e) was required to electrodeposit all of the Zn and…

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Q: The reaction occurring in the cell in which Al2O3 and aluminum salts are electrolyzed is Al³+ (aq) +…

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Q: Balance the following redox reaction in basic solution.   Fe(OH)3(s)   +   OCl−(aq)   →…

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Q: 19 In acidic conditions, manganate(VII) ions are reduced to manganese(II) ions, Mn²+. In neutral…

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Q: If a current is flowing from a battery that's used to electroplate an object with silver, how do I…

A: Given:1.45 A.hr = 1.45 amp current per hour.

Q: What is the reducing agent in the following redox reaction? I2(aq) + 2Na2S2O3(aq) → Na2S4O6(aq) +…

A: Titrimetry and electrochemistry.

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A:

Q: Balance the following redox reaction in basic solution. 3+ Cr(OH)3(s) + Fe³+ (aq) 2+ Cro(aq)+ Fe²+…

A: Answer:

Q: Given the following redox reaction:  2Ag+(aq) + Cu(s) → 2Ag(s) + Cu+2(aq) Write the balanced…

A:

Q: Complete and balance the following redox reaction in acidic solution. Be sure to include the proper…

A: Answer:When during a chemical reaction oxidation and reduction take place simultaneously, then such…

Q: A total of 1.543 F of electricity (1 F = 1 mol e¯) was required to electrodeposit all of the Zn and…

A: ZnSO4 and CoSO4 both have divalent metal ions as, Zn2+ and Co2+.  (Here M= metal)So, 2F electricity…

Q: Balance the following redox reaction in acidic solution using the half reactions method. CuS (s) +…

A:

Q: Write a balanced chemical equation (including states of matter) for an electrochemical cell that has…

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Q: How many minutes does it take to plate 228.6 g of chromium onto a car part using 19.24 A of current?…

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Q: Balance the following skeletal reaction in acidic solution. Be sure to include “1” in the blank if…

A: A redox reaction is balanced by balancing the mass and charge. Hence the number of atoms of all the…

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.