Calculate the mass of Ag metal generated when Ag(NO3)(aq) is electrolysed for 20.5 minutes with a current of 2.28 A. Give your answer to 3 significant figures.

Q: Consider the following cell: |Zn (s) | Ca2* (aq) , so3²" (aq) || Hg2+ (aq) , F° (aq) | Pt (s) | a)…

A: In a cell notation, the left side represent anode reaction or oxidation-half reaction, and the right…

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

A: Answer: 174.0

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: Faraday’s first law of electrolysis:                 The mass of the substance deposited at the…

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: Faraday's first law of electrolysis states that the mass of substance deposited is directly…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

A:

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: How long (in hours) must a current of 4.61 amps be passed to produce 79.5 g of copper metal from a…

A: Given:: Current i= 4.61 A  Mass of Cu = 79.5 g  Molar mass of Cu= 63.55 g mol-1 Time t= ?

Q: Manganese dioxide (MnO2) for use in dry cell batteries is made by electrolyzing solutions of Mn2*…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn"…

A: The reaction given is Hence in the above reaction, Sn2+ is being reduced to Sn and Ba is being…

Q: A current of 0.500 A flows through a cell containing Cd(II) for 10.0 minutes. Calculate the maximum…

A: Current Strength = 0.500 A time = 10 min         = 10 × 60 sec                               (As, 1…

Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: Consider a galvanic cell based on the reaction Zn + MnO4→ Zn²* + Mn²+ in acidic solution. Calculate…

A:

Q: Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction:…

A:

Q: Two half-reactions of an electrochemical cell are given below :MnO–4 (aq) + 8H+ (aq) + 5e– → Mn2+…

A: Half-reaction is a part of redox reaction. It can be reduction half-reation or oxidation…

Q: The galvanic cell Zn(s) | Zn2+(aq) | | Ni2+(aq)| Ni(s) is constructed using a completely immersed…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

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: Suppose 220. mmol of electrons must be transported from one side of an electrochemical cell to…

A: Given  mmol of electrons = 220  Time = 214 s  We have to calculate current

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Since in the above reaction we can see that 1 mole of Cl2 is produced with 2 moles of electrons…

Q: Consider the following cell: | Zn (s) | Ca2* (aq), so32" (aq) || Hg2+ (aq) , F" (aq) | Pt (s) | a)…

A: In a cell notation, the left side represents the oxidation half-reaction taking place at anode,…

Q: A solution of NaCl is neutral, with an expected PH of 7. If electrolysis was carried out on 500 mL…

A:

Q: Electrolysis of a solution of Zn(NO3)2 (aq) to give zinc metal is carried out using a current of…

A: The expression for the mass of metal deposited is given as:

Q: suppose a current of 0.510 A flows through a copper wire for 281. seconds, calculate how many moles…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Sn…

A: The cell reaction taking place is given as, => Sn2+ (aq) + Ba (s) -------> Sn (s) + Ba2+ (aq)…

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: It is given that MgCl2 is electrolysed and a current of 12.4 A is passed for 1h.

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

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

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr** (aq) +…

A: Given reaction is ,           2Cr3+(aq) + 3Ca(s)----> 2 Cr(s) +3 Ca2+(aq) Nernst equation for the…

Q: Copper can be electroplated at the cathode of an electrolytic cell by the half-reaction: Cur"(aq) +…

A: Given, The mass of copper is 325 mg. The current is 5.6 A. The given reaction is,

Q: Enter your answer in the provided box. The MnO, used in alkaline batteries can be produced by an…

A: Please find the answer attached here as handwritten note.

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

A:

Q: How long ( hours) would it take to unload 0.433 moles of vibranium (Vb) metal during electrolysis of…

A: We have to calculate time needed for electrolysis  Molar mass of Tr not provided so only 1st…

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

A: The electrolysis of water produces oxygen. Since the O is in 2- oxidation state in water initially…

Q: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: Suppose a current of 0.590 A flows through a copper wire for 154. seconds. Calculate how many moles…

A: Given, Current (I) = 0.590 A Time (t) = 154. second Moles of electron transfer through the wire = ?

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3Cu (aq)…

A: The given redox reaction is,                                   3 Cu2+(aq) + 2 Al (s) ----> 3…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr* (aq)…

A: The reaction given is Hence in the above reaction, Cr3+ is being reduced to Cr and Ca is being…

Q: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

Q: You pass a 2.5 amp current through an aqueous solution of aluminum nitrate for 5 hours. How many…

A: Aluminium nitrate Al(NO3)3 has Al3+ ions Al3+ + 3 e-  -----> Al So to reduce 1 mole Al3+ ions to…

Q: Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²* (ag)…

A: The reaction given is Hence in the above reaction, Cu2+ is being reduced to Cu and Zn is being…

Q: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a…

A: The given equation is, The anode reaction of given cell is, The cathode reaction of given cell is,…

Q: A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell…

A: Given : Current passed = 0.25 A And time = 1 min F=96500 C/mol

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2* (aq)+…

A: The cell reaction taking place is given as, => 3 Cu2+ (aq) + 2 Al (s) -------> 3 Cu (s) + 2…

Q: Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction…

A: The balanced redox reaction can be written as: MnO4- + 8H+ + 5e-  →  Mn2+ + 4H2O (Reduction)5Ce3+  →…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu*…

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.