Write a balanced net ionic equation for the overall cell reaction repre- sented by (a) Cd Cd²+ || Sb³+ | Sb (b) Pt| Cu*, Cu²+ || Mg²+ | Mg 2.

Q: A student measures Ecell of a concentration cell created by having the saturated solution of AgBr on…

A: According to the guidelines, we will solve the first 3 parts. If you want any other part also…

Q: 6b. How long does it take to deposit a coating of gold 1.00 picometers thick on a disk-shaped…

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: How many grams of Pb would be deposited from an aqueous solution of Pb 2+ with a current of 1.828 A…

A:

Q: Complete and balance the following half-reaction in basic solution. Be sure to include the proper…

A: Thank you,Please rate my response.

Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: Give the cell voltage of the following cell Au | 1.0 M AUNO3 || 1.0 M AgNO3 |Ag o Li | 1.0 M LİNO3…

A: We need to find cell potential of the given cell notations.

Q: Consider the following redox reaction: Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq). How many moles of…

A: In the given reaction we can see that the Ag+ is being reduced to the Ag and Fe2+ is being oxidised…

Q: X(s)|X3+ (2.04 M) || Mn O4 1 minus (1.62 M)|Mn2+ (0.25 M)|H+ (2.64 M) The reduction potential for…

A: Given   The concentration of X3+ is 2.04 M. The concentration of MnO4- is 1.62 M. The concentration…

Q: 5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4…

A:

Q: Consider the following cell: | Zn (s) | Ca²* (aq) , SO3² (aq) || Hg²* (aq) , F` (aq) | Pt (s) | a)…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: 3. How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn²+ (aq) if the…

A:

Q: A student measures Ecell of a concentration cell created by having the saturated solution of AgBr on…

A:

Q: How many grams of Ag would be deposited from an aqueous solution of Ag+ with a current of 2.534 A…

A: Molar mass of Ag = 108g/mol Reaction takes place:- Ag+ + e-  ------> Ag  current , I = 2.534 A…

Q: Zn(s)| Zn²*(0.85 M) || Cu²*(1.10 M) | Cu(s) Zn(s)| Zn²*(1.05 M) || Cu²“(0.75 M)| Cu(s) Cell B a) Do…

A: To determine: (a) Direction of electron flow. (b) Ion concentrations in the half-cells at the point…

Q: Chloride ions are added to the Ag|Ag+ half-cell of the cell Ag|Ag+||Cu2+|Cu to precipitate AgCl (s).…

A:

Q: The condensed cell diagram for the reaction occurring in silver–zinc button batteries is  (-) Zn(s)…

A: This question belongs to Electrochemistry. The condensed cell diagram for the reaction occurring in…

Q: How many grams of indium may be formed by the passage of 6.73 amps for 2.55 hours through an…

A: Given, Current (I) = 6.73 A Time (t) = 2.55 hours = 2.55 × 60 × 60 s = 9180 s mass (in grams) of…

Q: How many seconds are required to deposit 0.145 grams of zinc metal from a solution that contains Zn*…

A: Answer :-  t = 447 (s) The time required to deposit 0.145 g of Zn metal from a Zn2+ solution when…

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 grams of thallium may be formed by the passage of 7,438 amps for 3.04 hours through an…

A:

Q: The enzyme hydrogenase carries out the reduction of hydronium ions to molecular hydrogen: 2H3O++…

A: The given reaction is:

Q: If you have the reaction Fe3+ + 3e- -> Fe, how many grams of Fe will result if you apply a current…

A: Faradays first  law of electrolysis , the amount of substance  deposited at cathode   is directly…

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: 4. Write the overall net ionic equations for the following voltaic cells: (a)…

A: (a)  Given,  Zn(s) Zn²+ (aq)||Fe²+ (aq)|Fe(s) Anode reaction;  Zn(s) -----> Zn²+(aq) + 2e-…

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.