What mass of rhodium (Rh) metal will be deposited from a solution of Rh3+ ions by running electrical current through the solution at 0.500 A for 120.0 minutes?

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

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Q: >Why do some electrochemical cells employ inert electrodes such as platinum?

A: In some redox reactions, may be one of the reactant or product and sometimes both reactant and…

Q: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

A:

Q: Based on standard reduction potentials, would you expect copper metal to oxidize under standard…

A: The value of E˚cell is calculated as shown below: Here, E cell is the standard potential of the…

Q: How many grams of chromium metal can be deposited using an electrolytic cell with an electrolyte…

A: Given : Current = 8.30 A  Time = 6 min = 6 X 60 s = 360 s  And the salt given is CrCl3.

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

A: Amount of charge (Q) = I . t  where I = current and t = time

Q: A concentration cell similar to the one shown is composed of two Mg electrodes and solutions of…

A: Oxidation is lose of electrons. Reduction is gain of electrons. Reactions where oxidation and…

Q: How many hours does it take to form 15.0 L of O, measured at 750 torr and 30°C from water by passing…

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Q: How many grams of magnesium metal will be deposited from a solution that contains Mg2+ ions if a…

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Q: A concentration cell similar to the one shown is composed of two Mn electrodes and solutions of…

A: Concentration cells use same electrode but the concentration of electrolytic solution varies. They…

Q: What mass of copper , in mg , can be deposited from copper (II) sulfate solution using a current of…

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Q: The standard reduction potential of a chromium electrode is -0.74 volts when chromium is reduced…

A: +1.59

Q: Metallic magnesium can be made by the electrolysis of molten MgCl2. (a) What mass of Mg is formed by…

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Q: In the commercial production of sodium metal by electrolysis, the cell operates at 7.0 V and a…

A: The faraday's first law explains that the quantity of any species deposited is directly proportional…

Q: What are Standard Reduction Potentials?

A: Standard reduction potentials has to be defined.

Q: Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is…

A: The standard reduction potential is measured under the following conditions as the 298 K…

Q: A. If the measured cell potential is 1.800V, what is the concentration of Au3+? B. How long will it…

A: Here we have to determine the concentration of Au+3 of the galvanic cell and mass of gold…

Q: How much time (in hours) is required to plate out 25.0 g of gold metal from a solution of Au(NO3)3…

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Q: A solution containing a 3+ metal ion is electrolyzed by a current of 5.0 A for 10 minutes. What is…

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Q: What mass of Cu(s) is electroplated by running 12.5 A of current through a Cu 2+ (aq) solution for…

A: We have to calculate the mass of Cu(s) is electroplated : First, we will write down all the given…

Q: What volume of chlorine gas at standard temperature and pressure is evolved when a solution of MgCl2…

A: Provided time=1hour Molar mass of Cl2=70.906g/mol Let w gram Cl2 evolve So provided time…

Q: Calculate the standard potential, E, for this reaction from its equilibrium constant at 298 K. X(s)…

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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: 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: 4.) What mass of silver can be plated onto an object in 45 minutes at 9.0 A of current?

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Q: Calculate the time required to precipitate 200 milligrams of copper by electrolysis of an acidic…

A: By 1F of charge 1 equivalent of metal can be deposited .

Q: What mass (in grams) of nickel could be electroplated from a solution of nickel(II) chloride by a…

A: From Faraday's first law of electrolysis, the weight of a chemical substance(w) deposited at an…

Q: A concentration cell similar to the one shown is composed of two Mg electrodes and solutions of…

A: A electrochemical cell is used is used convert chemical energy to electrical energy it involves  a…

Q: Explain Standard Electrode Potentials?

A: If the temperature is 298 K and the pressure is 1 atm,then these are known to be the standard…

Q: An aqueous solution contains a mixture of cations at the following concentrations.…

A: An aqueous solution containing a mixture of three cations, for which the order of reduction is to be…

Q: Determine the mass of Sodium( Na) produced when a 11 amp current flows for 4 hr through a cell…

A: We have given Determine the mass of Sodium(Na) produced when a 11 amp current flows for 4 hr through…

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

A: According to Faraday's 1st law weight of the substance from in each electrolyte  W = ZIt where , W…

Q: How does lowering the concentration of the solution in the anode affect the cell potential? How does…

A: A galvanic cell is a electrochemical cell. It supply electric through a redox reaction. It  is…

Q: Calculate the cell potential given the standard reduction potentials for the half reactions of the…

A: Solution: We know at cathode reduction reaction occurs, so the half cell having highest value of…

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: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A:

Q: What period of time (in hours) is required to produce 1.00mol of chlorine using a current of 5.00A?

A: A numerical problem based on Faraday's law, which is to be accomplished.

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: How much silver was there in the solution if all the silver was removed as Ag metal by electrolysis…

A: Given, Time (t) = 0.60 hr = 2160 s Current (I) = 1.00 mA = 1.00 × 10-3 A Amount (in grams) of silver…

Q: A cell has a standard emf of+ 0.134 V at 298 K.

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Q: What do you mean by ( i) negative standard electrode potential and(ii) positive standard electrode…

A: Standard electrode potential is defined as the potential of the electrode at the standard conditions…

Q: Copper metal (63.546 g/mol) is purified by electrolysis. How much copper metal (in grams) could be…

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Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given data:  Current = 4.57 A  Cr deposited = 14.5 g  Molar mass of Cr = 52 g.mol-  CrCl3  ==>…

Q: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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Q: How long will it take to deposit 0.0047 mol of gold by electrolysis of KAuCl4 using a constant…

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Q: At 298 K a cell reaction has a standard cell potential of+0.17 V. The equilibrium constant for the…

A: At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the…

Q: How many hours does it take to form 15.0 L of O2 measured at 750 torr and 30°C from water by passing…

A: According to Faraday's first law ,when current is passed through an electrolytic solution, the…

Q: How much time is needed to deposit 1.0 g of chromium metal from an aqueous solution of CrCl3 using a…

A: Faraday's law of electrolysis draws a relationship between the amount of substance deposited by an…

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.