Why is it that from nails and bolts to bridges, to roofing and framing components, countless items are made of galvanized iron and not from pure iron?

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

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Q: Why do reference electrodes serve as a probe to measure relative reduction potentials or even detect…

A: Answer - Reference electrodes - A reference electrode is an electrode which has a stable and…

Q: The chemistry of corrosion of iron is essentially an electrochemical phenomenon. Explain the…

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Q: What voltage can theoretically be achieved in a battery in which lithium metal is oxidized and…

A: Theoretically occurring reactions at anode and cathode are as follows:

Q: Based on standard reduction potentials, would you expect copper metal to oxidize under standard…

A: The value of E˚cell is calculated as shown below: Here, E cell is the standard potential of the…

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: Nickel and silver rods are placed in a solution of nickel ion and silver ion solutions of…

A: The considered cell is made of nickel and silver electrodes.

Q: Using data from the Standard Reduction Potentials table, place the following in order of increasing…

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Q: Suppose you are given a 1M solution of SnCl2 and another 1M solution of MgCl2. Leaving the…

A: The question is based on concept of redox chemistry. we have to determine the concentration of tin…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 4.65…

A: Question is based on first law Faraday's law of electrolytes. i.e., amount of substance deposited is…

Q: 7. Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: cathode when coupled with a SHE in a galvanic cell. (Hint: What units are required Calculate the…

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Q: In an experiment similar to this one, a polished strip of Cu (s) was found to weigh 16.552 g. This…

A: Given : Mass of Cu before electrolysis = 16.552 g Current passed = 0.887 A Time = 26 min = 26 X 60 =…

Q: 1. A constant current of 90 mA is applied to an electrochemical cell for 22 minutes. What is the…

A: The charge transport in a unit time is known as electric current. The current is calculated by using…

Q: A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

A: The Faraday’s first law of electrolysis state that the mass of the substance  deposited at any…

Q: Galvanized iron is steel sheet that has been coated with zinc; “tin” cans are made of steel sheet…

A: To discuss: The functions of coating? Electrochemistry of corrosion reactions?

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

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Q: Calculate the cell potential, ε for this galvanic cell and ΔG for the cell reaction these…

A: The cell reaction is Overall reaction is given by,

Q: Between the galvanic couple Pb and Al, which metal is the cathode?

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Q: An electrochemical cell is constructed in which the silver ions in silver chloride are reduced to…

A: Given,  A current of 0.500 A is passed through the cell for 101 minutes. The mass of copper metal…

Q: This process is done in an alkaline environment, and one of the solutions used for this process is…

A: Given, galvanization process is done by passing electricity through Na2Zn(OH)4. What is the balanced…

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: If a galvanic cell is constructed using Au3+ and Al3+, which ion will most likely be in the anode?

A: Reduction Addition of electron is called reduction Oxidation Removal of electron is called oxidation

Q: Identify the reaction at the anode, reaction at the cathode, the overall reaction, and the…

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Q: Please make a sketch in the electrolysis of aqueous potassium bromide and indicate the anode and…

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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: Why EMF of the cell increases when the concentration of the solution at the anode decreases? Why EMF…

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Q: b. Assuming the two half cells operate at standard conditions, calculate the standard reduction…

A: Recall the given half-cell reactions :                        HgO s  +  H2O l  +  2 e-  →  Hg l  +…

Q: How does Galvanisation check rusting of iron?

A: Rusting of iron means formation of a layer of iron oxides on the surface of iron objects. This…

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: d). For the electrochemical cell, Fe(s) | Feaq) || Cu aq)| Cu'(aq) | Pt(s), determine the…

A: Analyzing the given cell shows that it contain two half reactions depicted as below,

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.35…

A: moles of electrons  =6.2x1018 x2.35x140x60/6.022x1023 =20454 x 10-5 =0.2 Moles of electron = number…

Q: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: In the electrolysis of an aqueous solution of Na2SO4, what reactions occur at the anode and the…

A: Explanation to the correct answer is given below

Q: How many minutes would it take to plate 12g of silver from an aqueous Ag(l) solution using a current…

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Q: A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M iron(II) ion solution…

A: Answer: the standard potential for this cell at 25°C is 1.96 V.

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

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Q: A solution of CuSO4 is electrolysis for 10 minutes with a current of 1.5 amperes. What is the mass…

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Q: How much silver was there in the solution if all the silver was removed as Ag metal by electrolysis…

A: Given, Time (t) = 0.60 hr = 2160 s Current (I) = 1.00 mA = 1.00 × 10-3 A Amount (in grams) of silver…

Q: Galvanized iron is steel sheet that has been coated with zinc,tin cans are made of steel sheet…

A: A question based on electrochemistry, which is to be accomplished.

Q: how many minutes are required to plate 10.0g of nickel metal from a solution of NiSO4, if the…

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Q: What mass of gold is produced when 15.2 A of current are passed through a gold solution for 25.0 min

A: Given information: Current (I) = 15.2 A Time (t) = 25.0 min

Q: If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how…

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Q: A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper II)…

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Q: products

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Q: identify the reaction at the anode, reaction at the cathode, the overall reaction, and the…

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Q: Copper(I) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with…

A: Answer :- 1.45 × 1012  The equilibrium constant (K) at 25°C for the given reaction = 1.45 × 1012…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 3.75…

A: In the electrolysis process, the grams of Chlorine gas generated is calculated using,

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.