What is the potential of a concentration cell at 25.0 °C if it consists of copper electrodes dipping into two different solutions of Cu(NO3)2, one with a concentration of 0.015 M and the other with a concentration of 0.50 M? What would be the potential of the cell if the temperature of the cell were 75 °C?

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: >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: The equilibrium constant, K, was found to be 3.8 x108 at 25°C for the following reaction, 2X(s) +…

A: For the given reaction:  2X(s) +  3Y2+(aq)  →2X3+  + 3Y(s) As the charges are equal on both sides.…

Q: Use the tabulated electrode potentials to calculate K for the oxidation of iron by H++ (at 25°C):…

A:

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by…

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

A: Given, in anode Cr2+ was oxidized to Cr3+ In cathode, Cd2+ was reduced to Cd Concentration of…

Q: NO3 + H* + Zn → Zn²+ + NO2 + H2O

A: Given skeletal equation is: NO3-+H+ +Zn →Zn2++NO2 +H2O Calculate its standard cell potential(Eo) and…

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

A:

Q: 10. Calculate the potential of the following cells: a) a galvanic cell consisting of a lead…

A: Given:  Pb2+ =0.0848 MZn2+=0.1364 M TiO2+ =0.00146 M Ti3+ =0.02723

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

A:

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: Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate…

A:

Q: Cl2 + Br → Ch + Br2

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

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

A:

Q: How much Ca will be produced in an electrolytic cell of molten CaCl2 if a current of 0.452 A is…

A:

Q: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question.   A…

Q: Calculate the Gibbs free energy, AG°, for a galvanic cell whose two half-reactions: Mt3+ (aq) +3…

A: Mt is getting reduced and R is getting oxidized in the above reaction. Electrode potential at…

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: Write the cell notation for an electrochemical cell consisting of an anode where H2 (g) is oxidized…

A:

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) Fe2*(1.00 M) + H2(g)(1.00 atm) If the cell…

A: By applying formula Ecell = E•cell - 0.0591/2 . Log[Fe2+]| [H+]2  At 25 degree Celsius

Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

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: The following cell Ag | Ag+(0.10M) || Ag+(1.0M) | Ag is a concentration cell and is capable of…

A:

Q: Write the cell notation for an electrochemical cell consisting of an anode where H2 (g) is oxidized…

A:

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

A: (a)

Q: Consider the following cell reaction: Mn(s) + 2 H+(? M) Mn2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Given data : Mn(s) + 2 H+(_____M) gives  Mn2+(1.00 M) + H2(g)(1.00 atm)the cell potential (E cell…

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

A:

Q: What is the cell potential for the following reaction at room temperature?                Al(s) │…

A: At anode half cell.Al(s)→Al3++3e-..........1At cathode half cell.Cu2++2e-→Cu(s)........2multiplying…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr2+ (aq) is…

A:

Q: 4. In a process called flash electroplating, a current of 2.5 x 10'A passes through an electrolytic…

A:

Q: Calculate the actual cell potential if you have a 1 M solution of MgSO4, but only a 0.5 M solution…

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: Consider the following cell reaction: Mn(s) + 2 H*(? M) –→MN2*(1.00 M) + H2(g)(1.00 atm) If the cell…

A:

Q: Consider the following cell reaction: Co(s) + 2 H*(? M) Co2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Here we are required to find the pH of hydrogen electrode

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: Consider the following cell reaction: Fe(s) + 2 H*(? M) –Fe²*(1.00 M) + H>(g)(1.00 atm) If the cell…

A:

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) Fe"(1.00 M) + H2(g)(1.00 atm) 2+ If the cell…

A: We wil first write nernst equation, and then calculate pH of solution.

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

A:

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

A: Cell notation is a way to represent an electrochemical cell with anode and cathodes.

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

A: A numerical problem about galvanic cell constructed using two Hydrogen electrodes.

Q: How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: Given, m = 9.38g I= 23.2A

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: What is the maximum electrical work that can be obtained from 6.54 g of zinc metal that reacts in a…

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: An electrochemical cell consists of a silver metal electrode immersed in a solution with[Ag+]  = 1.0…

A: The given parameters are: [Ag+]  = 1.0 M molarity of NH3 = 5.0 M  [Cu(NH3)42+] = 0.020 M…

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.