A voltaic cell is constructed with two silver–silver chloride electrodes, each of which is based on the following half-reaction: AgCl1s2 + e- ¡ Ag1s2 + Cl -1aq2 The two half-cells have 3Cl -4 = 0.0150 M and 3Cl -4= 2.55 M, respectively. (a) Which electrode is the cathode of the cell?

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

A: Given-> Concentration of VO2+ = 3.63 M Concentration of H+ = 1.38 M Concentration of VO2+ = 0.607…

Q: 2. Calculate the potential of the following two half-cells that are connected by a salt bridge: a…

A: In galvanic cell redox reaction occur  Here We are required to find the potential of the given cell…

Q: A standard galvanic cell has a silver electrode in a .02M solution of Ag2SO4 and a gold electrode in…

A: From the standard reduction value, it can be conclude that which one will be oxidized or reduced.…

Q: What is the pH of the solution in the cathode half-cell when PH2 = 1.0 atm, 3Zn2+4 in the anode…

A: The anodic half-reaction and cathodic half-reaction that occurred in the electrochemical cell are as…

Q: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

A: The electrode in which anode and cathode both are form by same metal, tat cell is known as…

Q: Two hydrogen concentration half-cells are combined into an electrochemical cell at 25 degrees…

A: Cell reactions will be : H+(aq)(?) + e- ---->1/2 H2(g)          Reduction reaction (Cathode)…

Q: A molten binary salt, Cal2, is electrolyzed. Write the half reactions that occur and identify which…

A: The binary salt given is CaI2  hence it has cation Ca2+ and anions I-

Q: A solution of a metal ion M 3+(aq) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: The given data contains,       current =5 A      time =10 min60s1 min=600s

Q: A galvanic cell is constructed that carries out the reaction 2Ag(s) + Cl2 (g) → 2Ag+(aq) + 2CI- (ag)…

A:

Q: 8. Which of the following is false? In a galvanic electrochemical cell the cathode is the place…

A: At equilibrium, the potential of cell reaches to zero. The reactions proceeds in forward and…

Q: A galvanic cell with a voltage of 1.3 V utilises the reaction: Zn + Cu2+ →→ Cu + Zn2+, as a source…

A: Given: The cell voltage is 1.3 V. The amount of Cu and Zn used is 6.3 g and 11 g, respectively.

Q: A student does an experiment to determine the molar solubility of lead(II) iodide. She constructs a…

A:

Q: Which of the following statement/s is/are false? The cathode reaction in an electrolytic cell is…

A: Given: statements 1.The cathode reaction in an electrolytic cell is the reduction half-reaction.…

Q: A galvanic cell is set up by making 1 M solutions of FeSO4 and ZnSO4, with an iron (Fe) electrode in…

A: Interpretation-E0cell value. Concept introduction- Equation of half cell reaction anode-…

Q: How long will an electrolytic cell containing a solution of cadmium(II) iodide need to run at a…

A:

Q: A common car battery consists of six identical cells each of which carries out the reaction:…

A:

Q: A student wishes to set up a voltaic cell that is a concentration cell made using two solutions of…

A: Concentration cell and cell potential calculation :

Q: A voltaic cell is constructed at 25 °C from a half-cell in which a nickel rod is dipped into a…

A: The voltaic cells are electrochemical cells which has an anode and cathode separated and is…

Q: Four voltaic cells are set u. In esch, one half-cell contaias a standaed hydrogen electrode (SIIE).…

A: SHE is a reference electrode that has a reduction potential of 0 V. The half-reaction for SHE…

Q: A concentration cell constructed from two hydrogen electrodes, both with PH2 = 1.00. One electrode…

A: Nernst equation is, E=E0cell-RTnF lnQ T= temperature in Kelvin. n = number of electrons involved. F…

Q: Consider a battery made from one half-cell that consists of a copper electrode in 1 M CuSO4 solution…

A: Every battery can be considered as voltaic cell. At anode, oxidation takes place and at cathode,…

Q: a galvanic cell is constructed from a standard hydrogen electrode and from another hydrogen…

A: Given, A galvanic cell is constructed from a standard hydrogen electrode and from another hydrogen…

Q: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated…

A:

Q: A galvanic cell consists of a Au electrode in a 1.0 M Au(NO3) 3 solution and a Ni electrode in a 1.0…

A:

Q: If the following half-cells are the right-hand electrode in a galvanic cell with a standard hydrogen…

A: Given information: a) Ag |AgI(sat’d), KI(0.0898 M) b) Pt |Sn2+(0.0893 M), Sn4+(0.215 M) c)…

Q: 13. You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a…

A: Data given: The concentration of Al(NO3)3 = 1 M The concentration of AgNO3 = 1 M The electrodes…

Q: Calculate the equilibrium constant at 25 C for the Daniell cell.

A: The Daniell cell is a galvanic cell which converts chemical energy into electrical energy. The…

Q: A voltaic cell consists of a strip of cadmium metal in a solution of Cd(NO3)2 in one beaker, and in…

A: Given : We have to tell which of the following will act as anode and cathode.

Q: Calculate the emf of the following cell Zn / Zn?* (0.01 M) // Cu²* (1 M) / Cu, what will happen when…

A: Given: The concentration of Zn2+ ions is 0.01 M. The concentration of Cu2+ ions is 1 M.…

Q: The following galvanic cell isconstructed at 273 K.Each aqueous phase reactant and product has a…

A:

Q: a. A second student tries to set up the experiment above, but mistakenly grabs a bottle of 0.1 M…

A: In the given electrochemical cell, tin will act as cathode and iron will act as anode. The Nernst…

Q: In an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

Q: reaction of this electrochemical cell at 25 C

A: From the given information,  Net Spontaneous cell reaction , Mg(s) + 2Ag+(aq.) -----> 2Ag(s) +…

Q: A much-studied cell in electrochemistry has the following cell notation: Ag(s) | AgCI(s) || HCl(aq)…

A: At anode, oxidation and at cathode , reduction takes place. For which half cell reactions can be…

Q: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

A: Given, The voltaic cell, Zn2+ - Zn When the two half-cells have [Zn2+] = 1.8 M     and[Zn2+] = 1.00…

Q: Consider an electrochemical cell constructed from the following half cells, linked by a KCI salt…

A:

Q: For the following electrolyte-concentration cell consisting of two cells back to back by electrodes,…

A: The given cell representation  is ,                          Pt ; H2, HCl (a1), AgCl(s), Ag | Ag,…

Q: Which of the following statements is true concerning the electrochemical cell described below at…

A: The given cell is a concentration with the standard emf, E°cell = 0 At anode: Cu →Cu2+ + 2e-At…

Q: Electroclytic process of determining molar mass. An electrolysis cell X3+ ions. When at a 5.45 A…

A: Molar mass is defined as the mass of 1 mole of substance. Its units are g/mol. In order to determine…

Q: A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 ∘C. The initial…

A: The Nernst equation is shown below: Where: Ecell = cell potential E0cell = standard cell potential…

Q: How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: current = 15.9 A  (given) Molar mass of copper = 63.55 g/mol   (given) Cu is having n factor of 2…

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free ener these…

A: The question is based on concept of electrochemistry. we have been given a cell. We have   to…

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

A:

Q: A voltaic cell is set up with an aluminum electrode in a 0.025 mol/L AlI(NO3)3 aqueous solution and…

A: A numerical problem based on determination of cell potential.

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.