A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell in that time? (F = 96,500 C/mol)

Q: Suppose a galvanic cell is established using the following cell reaction, Cu(s) + 2Ag+(0.100 M)…

A: Given, The cell reaction is: Cu(s) + 2Ag+(aq)(0.100 M) <-----> Cu2+(aq) (0.200 M) + 2Ag(s)…

Q: A current of 3.79 A is passed through a Sn(NO^), solution. How long, in hours, would this current…

A: Oxidation is the process that involved the loss of electrons and oxidized to cation.  Hence when a…

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

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Q: 3. A voltaic cell employs the redox reaction: 2 Fe³+ (aq) + 3Mg (s)→2Fe(s) + 3Mg²+ (aq) Calculate…

A: In voltaic cell, oxidation takes place at anode while reduction takes place at cathode.  As per…

Q: Chemistry Question

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Q: How many minutes will it take for a current of 10.4 A to deposit 4.06 g of gold from a solution of…

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Q: A current of 4.76 A is passed through a Fe(NO3)2 solution for 1.20 h. Calculate the charge that…

A: Current = 4.76 A Time = 1.20 h

Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

A: M2SO4(aq) gives M+(aq) and SO42-(aq) ions. In the given Galvanic cell, the electrode is the same in…

Q: what is the combination of electrodes that would generate the greatest voltage in a galvanic cell?

A: Answer: The greatest voltage occurs when the difference in the reactivity of the two metals is the…

Q: What will be the overall balanced reaction if you want to make a galvanic cell? What is the…

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Q: A battery can provide a current of 4.00 A at 1.60 V for 1.00 hr. How much energy (in kJ) is…

A: Given that a current of 4.00 A was provided by battery at 1.60 V. The power can be calculated as…

Q: When [Hg2+] = 1.37 M, the observed cell potential at 298 K for an electrochemical cell with the…

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Q: Arrange the following from lowest to highest entropy: O2 (g), SO2 (g), SO3(g), S(s). Assume 1 mole…

A: standard entropy of O2 (g) =205.0 J/K mol standard entropy of SO2 (g) = 248.223 J/K mol standard…

Q: A battery can provide a current of 2.20 A at 1.00 V for 8.00 hr. How much energy (in kJ) is…

A: Given information,Battery provides a current 2.20 A at 1.00 V for 8.00 hr.Calculate the power,

Q: A redox process is found to have a K of 3.15 x 10° at 25 °C. What is AG° for this process at 25 °C?…

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Q: A certain metal M forms a soluble nitrate salt M M(NO3)₂. Suppose the left half cell of a galvanic…

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Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

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Q: A current of 5.83 A is passed through a Fe(NO3)2 solution for 1.60 h. How much iron is plated out of…

A: According to Faraday's law of electrolysis, the amount of substance deposited on an electrode is…

Q: 6. Calculate the standard cell potential for the following electrochemical cell. Cu" (aq) + Fe (s)…

A: Reduction potential of Cu2+ to Cu is 0.34V Reduction potential of Fe2+ to Fe is -0.41V In the given…

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A: As per the given information, this is basically concentration cell,where all the cell working due to…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: Galvanic cell consists of two half cell, the left half cell is called anode and the right is called…

Q: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

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Q: A battery can provide a current of 2.60 A at 1.60 V for 1.50 hr. How much energy (in kJ) is…

A: Given data: Currect (c) = 2.60 A, Voltage (v) = 1.60 V, Time (t) = 1.50 hrs. Power is calculated as,…

Q: A current of 4.30 A is passed through a Pb(NO3)2 solution for 1.80 h. How much lead is plated out of…

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Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: In this question, we want to determine the standard reduction potential of the cell.  You can see…

Q: A certain metal M forms a soluble sulfate salt M2SO4 . Suppose the left half cell of a galvanic cell…

A: Answer:When solution of same electrolyte with different concentrations is used in each compartment…

Q: When building a galvanic cell, what is the importance of the molecule in the anode vs the cathode.…

A: Galvanic cell converts chemical energy into electrical energy. Here Zn rod is dipped in ZnSO4…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: Electrochemical cells that have same electrolyte in two half-cells but with difference in their…

Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

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Q: 5. a) What type of voltaic cell is constructed from half cells consisting of the same electrode…

A: An electrolytic cell is one which converts electrical energy to the chemical energy i.e. an external…

Q: A current of 3.33 A is passed through a Sn(NO3)₂ solution for 1.30 h. How much tin is plated out of…

A: We have to calculate mass of tin deposited on the plate

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e → X(s)…

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Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

A: Answer: Left electrode will be positive. The voltage shown by the voltameter is ≈0.10V (0.0977V).

Q: A battery can provide a current of 2.20 A at 1.40 V for 10.0 hr. How much energy (in kJ) is…

A: GIVEN: Current = 2.20 A Voltage = 1.40 V Time= 10.0 hr To CALCULATE: Energy (kJ)

Q: Calculate the actual cell potential if you have a 1 M solution of MgSO4, but only a 0.5 M solution…

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Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A: A numerical problem based on electrochemistry, which is to be accomplished.

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: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: The voltaic cell shown above has two identical zinc electrodes : The solution in half-cell A…

A: For concentration cell E°cell = 0. And Ecell is calculated by using nearst equation   Here cell with…

Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

A: Concentration of sulfate salt in left half-cell = 3.5 MConcentration of sulfate slat in the right…

Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

A: Answer:When same electrolyte solution with different concentration is used in each compartment then…

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A:

Q: A certain metal M forms a soluble nitrate salt M(NO3)₂. Suppose the left half cell of a galvanic…

A: In the given Galvanic cell,  the electrode is the same in both the half-cells which is the metal, M.…

Q: An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a.…

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Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

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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.