The hydrogen-oxygen fuel cell is described in the text. For the questions below, assume the following: Assume that the air is 20 % O₂ by volume and that all the O₂ is consumed in the cell. The other components of air do not affect the fuel-cell reactions. Assume ideal gas behavior. (a) What volume of H₂(g), stored at 25.0°C at a pressure of 135 atm, would be needed to run an electric motor drawing a current of 8.50 A for 3.00 hr ? L (b) What volume (in liters) of air at 25.0°C and 1.06 atm will have to pass into the cell per minute to run the motor ? L/min

Q: 5) A certain electrochemical cell has a cell potential of +0.12 V. Which of the following is a true…

A: Electrochemical cell or galvanic cell converts chemical energy into electrical energy. In galvanic…

Q: The hydrogen-oxygen fuel cell is described in the text. For the questions below, assume the…

A:

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: At cathode reduction takes place while at anode oxidation takes place.  Current (I) = 1.55 A  Time…

Q: A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

A: Given : Current = 7.1 A And time = 40 min = 40 X 60 = 2400 s…

Q: An electrolysis cell is set up with the cathode producing H₂ gas and with an unknown metal at the…

A: Electrolysis Electrolysis involves passing an electric current through either a molten salt or an…

Q: A current of 2.345 A passes through the cell shown for 45 minutes. What is the volume of the…

A: It is a term used in chemistry when a substance undergoes a reaction in which it ends up gaining an…

Q: Why does the electrolysis of an aqueous sodium chloride solu-tion produce hydrogen gas at the…

A: Electrolysis is a method of passing electric current through ionic or molten salt resulting in the…

Q: In an electrochemical cell, a metal anode lost 0.187 g while a total volume of 0.08633 L of hydrogen…

A: The pressure of dry hydrogen gas can be determined as, Barometric Pressure = Pressure of water vapor…

Q: An electrolysis cell contains a solution of 0.10 M NiSO4. The anode and cathode are both strips of…

A: Electrolysis is spitting of chemical decomposition of ionic substances due to passage of electric…

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: 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: Aluminum is produced from the electrolysis of aluminum oxide dissolved in molten cryolite.…

A:

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

A:

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: Liquid potassium chloride, KCl(l), is decomposed in an electrolytic cell to form potassium and…

A: Faraday's law of electrolysis It states that the amount of substance deposited at an electrode is…

Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

A:

Q: A Voltaic Cell (also known as a Galvanic Cell) is an electrochemical cell that uses spontaneous…

A: Note: We can solve first three parts of question. Given: Diagram and data is given To find: a)…

Q: Calculate the number of grams of aluminum produced in one hour by the electrolysis of molten…

A:

Q: Part A Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An…

A: We have find out the answer.

Q: an electrolytic cell produces aluminum from Ai2O3 at the rate of ten kilograms a day. assuming a…

A: Given: Mass of Al per day is 10 kg

Q: Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If…

A: Total current, I = 1.09 million Ampere                           = 1.09×106 Ampere Time, t = 3 hr…

Q: An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a day. Assuming a…

A: The formation of Al from Al2O3 is as follows: 2Al2O3(s)→4Al(s)+3O2(g) Calculation of no. of mol of…

Q: When chlorine gas is bubbled through an aqueous solution of NaBr, chloride ions and liquidbromine…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Write the anode and cathode reactions occurring in a commonly used mercury cell. How is the overall…

A: The anode and cathode reactions occurring in a commonly used mercury cell and the overall reaction…

Q: In an electrochemical cell, a metal anode lost 0.286 g while a total volume of 0.04854 L of hydrogen…

A:

Q: The hydrogen-oxygen fuel cell is described in the text. For the questions below, assume the…

A: (a) Given that : Temperature = 25.0 °C Pressure = 142 atm Current = 8.50 A Time = 3.00 hr

Q: In an electrochemical cell, a metal anode lost 0.259 g while a total volume of 0.08398 L of hydrogen…

A: Answer:Here:

Q: e e Inert Inert Electrode Na(l) Electrode Cl2(9) Molten NaCI CI- Na+ Anode Cathode

A:

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: When 1.00 mole of chlorine gas is reduced to chloride ions in an electrolytic cell, what charge (in…

A: Reduction of 1 mol of chlorine is given below, Number of moles of electrons is 2.

Q: Suppose we construct a galvanic cell by placing two identical platinum electrodes in two beakers…

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.