In a galvanic cell, one half-cell consists of gaseous chlorine bubbled over a platinum electrode at a pressure of 1.00 atm into a 1.00 M solution of NaCl. The second half-cell has a strip of solid gallium immersed in a 1.00 M Ga(NO3)3 solution. The initial cell potential is measured to be 1.918 V at25°C, and as the cell operates, the concentration of chloride ion is observed to increase.(a) Write balanced equations for the half-reactions at the anode and the cathode.(b) Calculate the standard reduction potential of a Ga3+ | Ga half-cell. Consult Appendix E for the reduction potential of the Cl2 | Cl- electrode

Q: A galvanic cell consists of a cathode with a cadmium electrode in a 0.252 M solution of Cd(NO3)2 and…

A: The concentration of cadmium ions at anode is equal to the concentration of cadmium nitrate solution…

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

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²* (aq)+…

A: The reaction given is, Cu2+aq+Zns→Cus+Zn2+aq Cu2+ is being reduced to Cu and Zn is being oxidised to…

Q: Balance the following reaction. Calculate the cell potential and the Gibbs free energy of the…

A: The questions are based on the concept of redox reactions.   Redox Reaction  are those reactions in…

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

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cu (s) is oxidized…

A: The cell notation for electrochemical celk is given below.

Q: Calculate the cell potential for the galvanic cell in which the reaction   Fe(s)+Au3+(aq)↽−−⇀…

A: Please find your solution below :

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: Cl2 + Br → Ch + Br2

A: The questions are based on the concept of redox reactions.   Redox Reaction  are those reactions in…

Q: How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: The balanced chemical equation for the reduction of copper is: Thus, for the production of 1 mole…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized…

A: At anode, oxidation takes place. At cathode, reduction takes place.

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: Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized…

A: electrochemical cell is a device which generates electrical energy from chemical emery , in…

Q: Write the cell diagram for a galvanic cell consisting of an Al electrode placed in a 1 M Al(NO3)3…

A: Given:-           Al electrode placed in IM AlNO33 solution          Ag electrode placed in IM…

Q: The salt bridge in a galvanic cell allows the soltuions in the half cells to remain electrically…

A: In this question, we have to choose the correct option regarding salt bridge.

Q: Calculate the cell potential for the galvanic cell in which the reaction   Fe(s)+Au3+(aq)↽−−⇀…

A: Answer:- This question is answered by using the simple concept of calculation of cell potential…

Q: For the following reactions, determine the standard cell potential, the cell potential, ΔG and ΔG°…

A: a)

Q: How long will it take to produce 78 g of Al metal by the reduction of Al* in an electrolytic cell…

A:

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: A fuel cell is constructed in which both electrodes make use of the oxidation of methane. The…

A: (a)

Q: The equilibrium constant for the reaction Zn(s) + Fe2+(aq)⇌ Zn2+(aq) + Fe(s) is 6.66 x 1010 at 25…

A:

Q: In a galvanic cell, a full redox reaction takes place, one half-reaction at each electrode. How is…

A:

Q: A galvanic cell consists of a Mg electrode in 1 M Mg(NO3)2 solution and a Ag electrode in 1 M AgNO3…

A: Given- Electrodes Mg  in 1 M Mg(NO3)2 solution Ag  in 1 M AgNO3 solution Temperature = 25 °C   To…

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

Q: In one process used for electroplating silver, a current of 10.23 A was passed through an…

A: Dear student, this question is related to electroplating process.

Q: Write the cell notation for an electrochemical cell consisting of an anode where Fe2+ (aq) is…

A:

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: ulate the potential of the following cells: a galvanic cell consisting of a lead electrode on the…

A:

Q: Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized…

A: In an electrochemical cell, the electrical energy is produced from the spontaneous cell reaction at…

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: [Cr2+] = 0.00190 M [Au3+] = 0.824 M ->Answer may differ slightly because values of standard…

Q: The dilute sulfuric acid solution is electrolyzed with platinum electrodes with a current of 1.25 A…

A: Volume of gases evolved can be calculated from the moles of gases evolved..

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: Write the cell notation for an electrochemical cell consisting of an anode where Co (s) is oxidized…

A:

Q: A fuel cell is constructed in which both electrodes make use of the oxidation of methane. The…

A:

Q: A galvanic cell with a measured standard cell potencial of 0.27 V is constructed using two beakers…

A: In the galvanic cell, the given reactions are: Cathode: Ni2+(aq)+ 2e-➡Ni(s) Anode:Ga(s)➡Ga3+ (aq) +…

Q: Calculate the standard cell potential produced by a galvanic cell consisting of a nickel electrode…

A:

Q: A voltaic cell employs the following redox reaction: 2 Fe³+ (aq) +3 Mg (s) → 2 Fe (s) +3 Mg²+ (aq)…

A: Given- 2Fe+3 (aq) + 3 Mg (s)  → 2Fe (s) + 3 Mg2+(aq)   Oxidation half reaction = 3 Mg (s) →3…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized…

A: In an electrochemical sell there is cathode and anode and the reaction takes place simultaneously .

Q: Write the cell notation for an electrochemical cell consisting of an anode where Fe2+ (aq) is…

A: Answer is explained below. According to the question,  At anode : Fe2+ (1M) | Fe3+ (1M) At cathode :…

Q: The electrolysis of an aqueous solution of potassium iodide, KI, results in the formation of…

A: Electrolysis: It is a chemical reaction that occurs when an electric current is conducted through a…

Q: Draw a galvanic cell consisting of a chromium and cobalt electrode and calculate the standard cell…

A:

Q: A galvanic cell is made up of one electrode consisting of a copper metal immersed in 0.00500 M…

A: Given,  A galvanic cell is made up of one electrode consisting of a copper metal immersed in 0.00500…

Q: Give the reason why it is necessary to use hydrogen as a standard to define the standard potential…

A: A standard electrode is an electrode used as a reference in electrochemical reactions and this…

Q: A voltaic cell (also called a galvanic cell) was constructed by connecting two beakers with a salt…

A: Given: Standard half-cell reduction potentials:Fe2+(aq)  +  2e-  ----->  Fe(s)     E o  =  -0.45…

Q: The anode compartment of a galvanic cell consists of a Zn anode immersed in 0.05M ZnCl2 The cathode…

A:

Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483…

A:

Q: Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker…

A: Interpretation - To write the half cell reaction that occurs at each electrode To check here which…

Q: What is the maximum electrical work obtainable from this cell when 0.150 g of Al is consumed?

A: Provided data :- E°cell = 1.63 V  Cell reaction :- Al(s) + Cr3+(aq) -> Cr(s) + Al3+(aq) It means…

Q: The oxidation of methanol, as described by the equation below, has a ΔG° value of -937.9 kJ/mol.…

A: Given Oxidation of Methanol 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)∆Gcell° = -937.9 kJ/mol =…

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.