How many grams of cobalt may be formed by the passage of 3.71 amps for 2.68 hours through an electrolytic cell that contains an aqueous cobaltous (Co(II)) salt.

Q: Explain what is a standard reduction potential, standard oxidation potential and standard cell…

A: Given We know about 1) standard reduction potential  2) standard oxidation potential 3) standard…

Q: How many grams of nickel remains in a 100 ml of 1.50 M NİCI4 solution if 3.0 ampere current is…

A: V = 100 ml = 0.1 L M = 1.50 M I = 3 Amp t = 1 hr = 60 x 60 = 3600 sec W = ? nf = 4 By using Faraday…

Q: Determine the mass of Sodium (Na) produced when a 373 amp current flows for 7 hr through a cell…

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Q: Write the cell diagram for the voltaic cell. You may assume it is constructed from metallic…

A: The reduction potential of Pd2+ to Pd is 0.915 V and Cr2+ to Cr is -0.89 V. Since the reduction…

Q: What electrochemistry principles are involved in the corrosion of metals and its prevention?

A: Corrosion : The deterioration or decay of a metal, because of its reaction with water or air is…

Q: A tin plated steel can corrode more quickly than an unplated steel can. In cases of galvanic…

A: a) The standard reduction potential of Sn2+ and Fe2+ are -0.13 V and -0.44 V respectively. Since…

Q: 1. What mass of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from…

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Q: explain why a galvanic cell can only work when the electrolyte solution remains electrically…

A: Galvanic cells also known as voltaic cells, are electrochemical cells in which spontaneous…

Q: Illustrate the features of Corrosion reactions?

A: ANSWERE IS DISCUSSED BELOW :

Q: (a) Write the possible oxidation and reduction half-reactions that occur when magnesium is immersed…

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Q: What are Standard Reduction Potentials?

A: Standard reduction potentials has to be defined.

Q: A 1.0 M solution of aluminum nitrate is placed in a beaker with a strip of aluminum metal. A 1.0 M…

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Q: Balance the following redox reaction that occurs under basic, aqueous conditions: NiO2 + Fe →…

A: To balance a redox reaction,follow the below mentioned steps: 1) Consider oxidation and reduction…

Q: Complete and balance the following half-reactions. In each case, indicate whether the half-reaction…

A: Many types of reactions are studied in chemistry like displacement reactions, addition reactions,…

Q: Which of the following reactions occurs at the cathode of an electrolytic cell containing molten…

A: Eleсtrоlysis invоlves the mоvement оf iоns tо the eleсtrоde. Sоlid-stаte dоes nоt аllоw the mоvement…

Q: How many grams of lead may be formed by the passage of 7,727 C through an electrolytic cell that…

A: The mass of any substance deposited via electrolysis is calculated using Faraday's first law of…

Q: y grams of radium can form by passing 278 C through an electrolytic cell

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Q: A redox reaction has an equilibrium constant of K = 0.055. What is true of AGn and Ea for this…

A: Redox reaction is where oxidation and reduction take place at the same time in the same reaction.

Q: 19.69 Calculate the standard cell potential of the following cell at 25°C.…

A: In the electrochemical cell notation, chromium electrode function as anode and mercury function as…

Q: Write the shorthand notation of the cell in question 3. If the standard reduction potential for…

A: The reaction is spontaneous with negative value of  ΔG◦ and positive value of E◦

Q: A group of galvanic cells a(n)... a) Battery b) Voltaic Cell c)Sickle Cell d) Electron Transport…

A: A group of galvanic cells:

Q: What mass of lead sulfate is formed in a lead-acid storage battery when 1.00 g of Pb undergoes…

A: The overall reaction in lead-acid storage battery is given below.

Q: Write the anode and cathode reactions that cause the corrosion of iron metal to aqueous iron(II)

A: Corrosion is a natural process that converts a refined metal into a more chemically stable form such…

Q: Define corrosion. Differentiate an anodic reaction from a cathodic reaction. What are the conditions…

A: Ans 1)  Corrosion is when refine metal convert into more stable form such as oxide, sulphide Or…

Q: 1. Write oxidation half-reactions for the metals Ag, Cu and Zn. Ag: Cu: Zn:

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Q: Calculate the concentration of HCI solution that has an H₂ pressure of 0.888 atm and gives an…

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Q: Predict which cation will be reduced first if the following mixture of molten salts undergoes…

A: The Cations in the given salts are, NaCl = Na+ CaCl2 = Ca2+ AgCl = Ag+

Q: What methods are used to reduce the corrosion of metals?

A: Corrosion is a naturally occurring process where a metal is converted into its metal oxide by…

Q: In a Galvanic cell, a salt bridge is often used. Explain why this is necessary. Describe the…

A: In a Galvanic cell, a salt bridge is often used to maintains electrical neutrality within the…

Q: How does lowering the concentration of the solution in the anode affect the cell potential? How does…

A: A galvanic cell is a electrochemical cell. It supply electric through a redox reaction. It  is…

Q: Using the provided standard reduction potentials, which of the following cells is an example of a…

A:

Q: Using the provided standard reduction potentials, which of the following cells is an example of a…

A: Galvanic cell converts chemical energy into electric energy It has zinc electrodes as anode.On anode…

Q: in an electrolytic cell, 0.5a of electricity is passed through molten chloride of iron and the…

A: Given :  Current I = 0.5 A  Time t = 4 hours = 4 * 3600 s = 14400 s  Mass of iron deposited = 1.39 g…

Q: grams of iron

A:

Q: Using the provided standard reduction potentials, which of the following cells is an example of a…

A: An electrochemical cell in which an electric current is generated from spontaneous reaction   Ex…

Q: Explain how a salt bridge can maintain electrical neutrality within the internal circuit of the…

A: Salt bridge is inverted U shaped glass tube filled with strong electrolyte (like NH4NO3) dissolved…

Q: Suppose a galvanic cell is established using the following cell reaction, Cu(s) +2Ag*(0.100 M)…

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Q: 12 The standard cell potential for the following galvanic cell is 0.71 V.…

A: Given- Standard cell potential of galvanic cell =0.71V Mg(s)|Mg2+(aq)||Al3+(aq)|Al  Equilibrium…

Q: Use the Potential-pH Diagram of Fe – H2O system to state the reactions the system undergoes and the…

A: Given : Use the potential-pH Diagram of Fe-H2O system to State the reactions the system undergoes…

Q: Using the provided standard reduction potentials, which of the following cells is an example of a…

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Q: Faraday constant. Suppose that after the electroplating was complete, you wiped the cathode copper…

A: Explanation to the correct answer is given below

Q: In what way does a galvanic cell becomes an electrolytic cell?

A: The galvanic cell become an electrolytic cell in the following way:-  As galvanic cells are…

Q: Complete and balance the following half-reaction in basic solution 5 X Cr(OH)3(s) → CrO42-(aq)

A: The given half cell reaction is: To balance, under basic medium, following steps are needed: First…

Q: Write the half reaction for the anode and the cathode in the galvanic cell For Silver and Zinc

A: The concept of half reactions is used to describe what occurs in a electrochemical cell ,such as a…

Q: A cell is constructed by immersing a strip of lead in a 1.0 M Pb(NO3)2 solution and a strip of…

A: Reduction occurs at cathode a d oxidation occurs at anode. We will answer this question by choosing…

Q: A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous…

A:

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.