An electrolysis cell contains a solution of 0.10 M NiSO4. The anode and cathode are both strips of Pt foil. Another electrolysis cell contains the same solution, but the electrodes are strips of Ni foil. In each case a current of 0.10 A flows through the cell for 10 hours.(a) Write a balanced equation for the chemical reaction that occurs at the             anode in each cell.(b) Calculate the mass, in grams, of the product formed at the anode in each       cell. (The product may be a gas, a solid, or an ionic species in solution.)

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

A:

Q: What mass of aluminum will be deposited in 1.00 hours by the electrolysis of molten AlCl 3 using a…

A: Electrolysis is the process of passing direct current through an electrolyte it produces chemical…

Q: During a period of discharge of a lead–acid battery, 402 gof Pb from the anode is converted into…

A: Overall cell reaction is Pb(s) + PbO2(s) + 2H+ (aq) + 2HSO4- → 2 PbSO4 + 2H2O Where, 1 mol of Pb is…

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: 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: A current of 12.0 A is passed through molten magnesium chloride for 14.0 h. How many moles of…

A: Given: Current = 12.0 A Time = 14.0 h

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: It took 116 hours to produce 603 g of metal X by performing electrolysis on molten XC13 with a…

A: From Faraday’s first law of electrolysis the quantity of charge is calculated as: Where, Q is…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 4.65…

A: Question is based on first law Faraday's law of electrolytes. i.e., amount of substance deposited is…

Q: 7. Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

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: A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

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

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: 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: Question three on photo

A: question is based on Faraday's first law of electrolysis. i.e., amount of substance deposited is…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 3.10…

A: Formation of Cl2 from NaCl is shown below,

Q: Elemental calcium is produced by the electrolysis of molten CaCl2. (a) What mass of calcium can be…

A: Given: Current applied  = 7.5 x 103 A Time of supply   = 48 h Efficiency of cell = 68%

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: Calculate the quantity indicated for each of the following electrolysis. a. The mass of Zn deposited…

A: The mass of zinc can be calculated by using Faraday's law of electrolysis.

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: Why is it that from nails and bolts to bridges, to roofing and framing components, countless items…

A:

Q: (4) When a metal of molar mass 207 g mol" is deposited by electrolysis, a current of 0.06 A flowing…

A: Convert the unit of time: 1 min=60 s66 min=66 min×60 s1 min=3960 s

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: Electrolysis of a solution of Zn(NO3)2(aq) to give zinc metal is carried out using a currentof 2.12…

A:

Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

A:

Q: How many milligrams of hydrogen can be produced by the electrolysis of water with a current of 0.308…

A: The electrolysis of water reaction producing hydrogen is  2 H+ + 2 e- -----> H2  Hence we can see…

Q: An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.35…

A: moles of electrons  =6.2x1018 x2.35x140x60/6.022x1023 =20454 x 10-5 =0.2 Moles of electron = number…

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: A copper rod was purified using an electrolysis method consisting of a 1.0 M solution of copper (II)…

A: The correct answer is given below ?

Q: Enter your answer in the provided box. Copper is purified by electrolysis. A 4.75-kg anode is used…

A: Given:  Mass of anode = 4.75 kg = 4750 gm  Current (I) = 37.8 A

Q: An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a day. Assuming a…

A: The formation of Al from Al2O3 is as follows: 2Al2O3(s)→4Al(s)+3O2(g) Calculation of no. of mol of…

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: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A:

Q: 7. How many grams of aluminum metal (26.982 g/mol) can be produced by the electrolysis of Al2O3…

A: In Al2O3, the oxidation number of Al is +3 and that of O is -2.  Hence uring electrolysis of Al2O3,…

Q: A solution of CuSO4 is electrolysis for 10 minutes with a current of 1.5 amperes. What is the mass…

A:

Q: During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on…

A: When a charge Q passes through a circuit the current through that circuit can be calculated by the…

Q: 4. A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper (II)…

A: Anode is the electrode on which oxidation takes place and Cathode is the electrode where reduction…

Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

A:

Q: A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper II)…

A:

Q: products

A:

Q: If a solution of CuCl2 is electrolyzed, what reaction will occur at the anode when the minimum…

A: In the electrolysis process, the cations move towards the cathode and the anions move towards the…

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

A: Faraday's first law of electrolysis It states that the mass of a substance deposited on any…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.30…

A: In the electrolysis process, the grams of Chlorine gas generated is calculated using,

Q: what mass, in g, of copper will be deposited from a solution of Cu^2+ by a current of 2.43 A in 7.52…

A:

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

A:

Q: a galvanic cell consists of a zinc electrode immersed in 0.1 M ZnSO4 solution and another zinc…

A:

Q: How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current…

A: Faraday's law of electrolysisAsW= Ite/FF= 965900 Ct=20 x 60 sece for copper if taken in copper…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 3.75…

A: In the electrolysis process, the grams of Chlorine gas generated is calculated using,

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.