H20 + H2SO4 O2(g). H2(g) Anode -Cathode + Voltage source Figure 17.20 Water decomposes into oxygen and hydrogen gas during electrolysis. Sulfuric acid was added to increase the concentration of hydrogen ions and the total number of ions in solution, but does not take part in the reaction. The volume of hydrogen gas collected is twice the volume of oxygen gas collected, due to the stoichiometry of the reaction.

Q: When a galvanic cell operates long enough, we notice as the electrodes undergo physical changes.…

A: Answer - galvanic cell  - A galvanic cell or voltaic cell, respectively, is an electrochemical cell…

Q: Indicate if each of the following statements is true of false. If false, rewrite it to make it a…

A:

Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A: Electric current : It is defined as the rate at which a particular charge flows. It is represented…

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

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

Q: A metallic object to be plated with copper is placed in a solution of CuSO.. What mass of copper…

A: Given,  Current, I = 0.22 amp  Time, t = 1.5 hours               = 5400 sec  Molar mass of Cu =…

Q: What mass of silver would plate onto the cathode if a current of 6.7 AA flowed through the cell for…

A:

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

A:

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: left half cell concentration = 3.00MRight half cell concentration = 15mMTemperature T= C + 274 =…

Q: In a separate electroplating experiment, if a 5.00 A current was used to electroplate a penny for…

A: Given : Current used = 5.00 A And time of current flow = 5.00 min = 5 X 60 = 300 s…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A:

Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

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

A:

Q: Explain the standard state reaction in Electrolysis of Water.

A: Following is the standard cell reaction in electrolysis of water.

Q: state and explain Faraday’s laws of electrolysis. What is Electrochemicalequivalent?

A: Faraday’s first law of electrolysis states that the mass of the substance accumulated or released at…

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A: To determine which electrode will be positive and the voltage that the voltmeter will show, we need…

Q: Is there a minimum standard reduction potential that the half-reaction used at the anode of this…

A: Well, we will use the given condition to calculate the reduction potential of anode. And we know…

Q: number of moles

A:

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: Given,  Concentration of MNO3 in left half = 22.5 mM  Concentration of MNO3 in right half = 4.50 M…

Q: electrochemical cell, a metal anode lost 0.123 g while a total volume of 0.09741 L of hydrogen gas…

A: Given data Volume of hydrogen gas = V = 0.09741 L Temperature = T =298 K  Barometric pressure =…

Q: the electromotive force of a galvanic cell constructed of a standard hydrogen electrode and a lead…

A: The electrode potential when the concentration of all the half cells involved is unity is called the…

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: Explain the different parts of a galvanic cell and also include its functions.

A: A galvanic cell is a device in which chemical energy is converted into electrical energy as a result…

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A: As per the given information, this is basically concentration cell,where all the cell working due to…

Q: A steady current of 10 A maintained for 1 hr deposits 12.2 g of zinc at the cathode. What is the…

A: Given,  I = 10 A.  t = 1 hr.  m = 12.2 gm.

Q: A current of 5.25 A is passed through an aqueous solution of copper(II) nitrate for 71.0 min. How…

A: An swer:- this question is answered by using the simple concept of calculation of mass of a metal…

Q: A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9…

A: We will use relation of mass and gm equivalent

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

A: Current (I) = 84 ATime (t) = 1 hour = 3600 s mass of Zinc metal produced = ?Note:Molar mass of Zinc…

Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

A: To find out the oxidation state, first find out the moles of e- and the moles of the rhodium. Then…

Q: A student was asked to set-up a galvanic cell in the laboratory. He used two copper electrodes, one…

A:

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: When same electrodes of same material used with different concentration then the Galvanic cell is…

Q: In an electrochemical cell, a metal anode lost 0.125 g while a total volume of 0.09055 L of hydrogen…

A: In an electrochemical cell, a metal anode lost 0.125 g while a total volume of 0.09055 L of hydrogen…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A:

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

A: Mass can be calculated as:-

Q: A constant current of 90 mA is passed for 22 minutes into an electrolysis cell. How much electrical…

A: Charge passing per unit time is known as  electric current.

Q: What mass (in g) of each product is produced in each of the following cells used for the…

A: "Since you have posted multiple questions, we will provide the solution only to the first two…

Q: How many milligrams of hydrogen can be produced by the electrolysis of water with a current of 0.308…

A: The electrolysis of water reaction producing hydrogen is  2 H+ + 2 e- -----> H2  Hence we can see…

Q: Why is important to physically separate the two half-reactions in a galvanic cell? So that the…

A: This is because,  The potential difference exists between two half cells and current is produced.…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A:

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: What is the time required to produce 45.0 g of Cl2 gas from Cl- using 50.0 A of current?

A: The oxidation reaction taking place will be  2 Cl- -------> Cl2 + 2 e-  Given : mass of Cl2 to…

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 calculated as follows

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A:

Q: grams of iron

A:

Q: What period of time (in hours) is required to produce 1.00mol of chlorine using a current of 5.00A?

A: A numerical problem based on Faraday's law, which is to be accomplished.

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.