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: 3. A galvanic cell is constructed comprising cadmium anode and nickel cathode: Cd (s) + Ni²+ (aq) →…

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Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: Ga3+ + 3e– ----> Ga(s)   Charge  = Current × time (s) = 0.830 A × (30.0 × 60 ) s = 1494 C

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: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

A:

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: An electrochemical bromate/bromide 3 Cu(s) + BrO3(aq) + 6 H*(aq) → 3 Cu2+ (aq) + Br¯(aq) + 3 H₂O(l)…

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Q: A steady current of 4A is maintained for 10.0 min. in a solution of silver nitrate. Find how much…

A: Given: Current = 4 A Time = 10.0 min Electrochemical equivalent of silver is 1.1180 x 10– 6 kg/C

Q: If the potential of a cell is 0.51 V at 25°C when [Zn2+(aq)]=0.111M and the pressure of the hydrogen…

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Q: Calculate the mass in grams of Zn deposited at the cathode in 42.5 minutes when 1.87A of current is…

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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: The electrolysis of TℓBr3 at high temperature produces thallium metal. If a constant electrical…

A: From Faradays first law, weight of the substance deposited, W = ZQ Z = E/F = equivalent…

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

A: Answer: Cell potential will be calculated using Nernst equation which is shown below:…

Q: of 15.00 x 10 mA flows for exactly two hours, calculate the number of tin atoms in the metal…

A: Using Faraday's law of electrolysis  Mass = Mit/nF Where, M = molar mass           i = current =…

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

A: The question is based on the concept of electrochemistry . we need to calculate cell potential of…

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

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

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

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

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Q: gallium (s) | 0.025 M gallium sulfate (aq) | 5 M KNO3 | 0.025 M copper (II) fluoride (aq) | copper…

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Q: An electrolysis cell contains a solution of 0.10 M NiSO4. The anode and cathode are both strips of…

A: Electrolysis is spitting of chemical decomposition of ionic substances due to passage of electric…

Q: Manganese metal can be produced industrially by electrolysis of MnO2. How many hours would it take…

A: The compound of manganese electrolysed is MnO2 having Mn4+ ion. Hence the electrolysis reaction to…

Q: An electrolytic cell produces aluminum from aluminum oxide, Al2O3. What mass of aluminum can be…

A: Applying formula w=Zit

Q: How many grams of silver metal will be deposited from a solution that contains Ag+ ions if a current…

A: Amount of current passed through the solution containing Ag+ ions = 0.695 A  Time of this current…

Q: impure

A: According to this law,  mass diposite on cathode is direactly proportion to the current.  So,…

Q: An aqueous solution of a platinum salt is electrolyzed for 1.00 hour using a current of 1.50 A to…

A: According to Faraday's law when a solution of an element is electrolysed then it will deposited.…

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

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Q: what mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution…

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Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:…

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Q: A current of 3.38 A3.38 A is passed through a Pb(NO3)2Pb(NO3)2 solution. How long, in hours, would…

A: Ans is 40.8min

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 moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq) using a…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2 MnO4 (aq)…

A: In the cell reaction, a spontaneous redox reaction occurs at the two different electrodes A redox…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2MnO4 (aq) +…

A:

Q: The electrolysis of AℓCℓ3 at high temperature produces aluminium metal. If a constant electrical…

A: Given: current = 10 × 103 mA Or current = 10 × 103 × 10-3 A Or current = 10 A And time = 1 hour =…

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Here we use the formula of metal deposited= ZIt , where Z is molecular weight, I= current, t= time…

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: 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…

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Q: Use the following standard reduction potentials to determine which species is the strongest reducing…

A: ->The species which has highest reduction potential that will get reduce itself and oxidize…

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: For the electrochemical cell, Cd(s) | Cd2*(aq) || Co2*(aq) | Co(s), determine the equilibrium…

A: In this question, we will determine the value of Keq ( equilibrium constant) value. First we will…

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

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: What is the potential of a concentration cell at 25.0 °C if it consists of copper electrodes dipping…

A: We have to find Ecell

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…

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.