How many hours are required to produce 5.00 g of chromium metal from an acidic solution of potassium dichromate using a current of 0.50 A? Cr203 + 14H+ + 12e → 2Cr(s) + 7H20

Q: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

A:

Q: How many seconds are required to deposit 0.137 grams of zinc metal from a solution that contains…

A: Mass of metal = I t × Mole Ratio × Atomic masd of metal / 96500  Where I = current  t = time

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

A: Answer: 174.0

Q: A current of 4.21 A is passed through a N i ( N O 3 ) 2 solution. How long, in hours, would this…

A: Current (I) = 4.21 A  Mass of nickel deposited (m) = 4.50 g

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3+ 3 Cu²+…

A: we have to calculate the cell potential

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) +…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2 Cr³+…

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

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

A: Step 1:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2VO₂ (aq) +…

A: The given cell reaction is- 2VO2+(aq) + 4H+(aq) + Fe(s)---> 2VO2+(aq) + 2H2O(l) + Fe2+(aq) [Fe2+]…

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

A:

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A:

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

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 long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

A:

Q: Calculate the mass of Ag metal generated when Ag(NO3)(aq) is electrolysed for 20.5 minutes with a…

A:

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: According to Faraday's Law: W=ZIt                         ...... (1) where w is the mass formed, I…

Q: rent of 1.88 x 10° ampere is passed thro olytic cell for 24 hours. Calculate the m s9% efficient 80%

A: Charge = current × time Q = I × t Mass = M × Q / n × F M is the molar mass n is the number of…

Q: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question.   A…

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

A: The oxidation and reduction half cells are as follows: Oxidation: 3Ca (s) →3 Ca+2     E0= -2.87…

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: In electrolysis cation is attracted towards cathode and anion is attracted towards to the anode.

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2103 (aq)…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2 Cr³+(aq)…

A: In the given galvanic cell ->Concentration of Cr3+ = [Cr3+(aq)] = 4.87 MConcentration of Ca2+ = […

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

A:

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

A: 1 F = 96500 C  Moles of chlorine = 1090 / 71 = 15.35 moles  Total charge = 2 × 15.35  F = 2 × 15.35…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2+ 2 Cr³+…

A: In an electrochemical cell, the chemical energy due to the chemical reactions is converted into…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr3+ (aq) +…

A: We can use Nerst Equation to solved the above problem.

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

A:

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: How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through…

A:

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

A: Current (I) = 84 ATime (t) = 1 hour = 3600 s mass of Zinc metal produced = ?Note:Molar mass of Zinc…

Q: A current of 2.90 A was applied to an electrolytic cell containing molten CdCl2 for 54 minutes.…

A: We have to calculate the mass of cadmium metal deposited when current passed is 2.90 A for 54…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

A: Step 1:  Calculate the cell voltage, using the Nernst equation. Ecell = E°cell - (RT/nF)lnQ where:-…

Q: What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given ,

Q: How many grams of nickel metal can be plated from 1.00M NISO4(aq), using a current of 3.00 A for…

A: Here mass of metal is calculated by using faraday's law

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2Cr³+…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: Calculate  the mass of Zinc deposited at the cathode in 26 minute when  1.87 Ampere of current is…

A: Electrodes are cathode and anode. The cathode is a negative electrode and the atom or ion undergoes…

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 many seconds are required to deposit 0.223 grams of lead metal from a solution that contains…

A: Given that, 0.223 grams of lead metal (Pb) is deposited from a solution that contains Pb2+ ions and…

Q: Write the balanced chemical equation for the spontaneous redox reaction. Include states of matter.…

A: The objective of the question is to-a) Write the balanced chemical equation.b) Determine the…

Q: What constant current would be needed for a copper cathode to accumulate 3.06 g of copper in 30 min.…

A: given- mass = 3.06 g. time = 30 min = 30 x60 = 1800 sec electrochemical equivalent of copper = 3.29…

Q: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) +…

A:

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

A:

Q: Determine the amount of time (in hours) that a 16.8 ampere current must be applied to a 2.0…

A: The objective of the question is to find out the time required to produce a certain amount of Zinc…

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

A: Given, Current flow (I) = 8.15mA = 8.15×10-3A Time = 12.6 min = 756S 2I–(aq) → I2(aq) + 2e(Anode…

Q: A current of 3.21 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

A: Given,a solution is:  Pb(NO3)2mass of lead = 7.50 gcurrent = 3.21 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.