A battery can provide a current of 2.40 A at 2.60 V for 4.50 hr. How much energy (in kJ) is produced?

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

A:

Q: Calculate the standard free-energy changed) for the reaction at 25°C Use the standard reduction…

A:

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: Faraday's first law of electrolysis states that the mass of substance deposited is directly…

Q: A current of 12.0 A is passed through molten magnesium chloride for 14.0 h. How many moles of…

A: Given: Current = 12.0 A Time = 14.0 h

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: A battery can provide a current of 4.00 A at 1.60 V for 1.00 hr. How much energy (in kJ) is…

A: Given that a current of 4.00 A was provided by battery at 1.60 V. The power can be calculated as…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: The reaction at Cathode is Lead sulphate is reduced to Lead. PbSO4 + 2e- ---> Pb + SO4 2-

Q: A battery can provide a current of 2.20 A at 1.00 V for 8.00 hr. How much energy (in kJ) is…

A: Given information,Battery provides a current 2.20 A at 1.00 V for 8.00 hr.Calculate the power,

Q: A voltaic cell was build upon the following redox reaction: 4 Ag (s) + O2 (g) + 4 H+ (aq) →4 Ag (s)…

A: if ∆G° is negative the reaction is spontaneous. if ∆G° is positive the reaction is non spontaneous.

Q: Consider a fuel cell that uses methane ("natural gas") as fuel. The reaction is…

A: Given: The reaction is CH4 + 2O2 → 2H2O + CO2

Q: A battery can provide a current of 2.60 A at 1.60 V for 1.50 hr. How much energy (in kJ) is…

A: Given data: Currect (c) = 2.60 A, Voltage (v) = 1.60 V, Time (t) = 1.50 hrs. Power is calculated as,…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: Given data,Current=29.0ATime=69.0sReaction at cathode;Pb2++2e-→Pb(s)

Q: When lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

A:

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

A:

Q: If 3.47 grams of silver have been plated on a piece of metal from an AgNO3 solution after 6.95…

A:

Q: Consider the following reaction: Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s), A Go = - 213kJ/mol Would it…

A: Answer :----The given reaction is :--Zn(s) + Cu2+ (aq) ------> Zn2+ (aq) + Cu(s) ΔGo = -213…

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: A battery can provide a current of 2.20 A at 1.40 V for 10.0 hr. How much energy (in kJ) is…

A: GIVEN: Current = 2.20 A Voltage = 1.40 V Time= 10.0 hr To CALCULATE: Energy (kJ)

Q: (a)  What quantity of charge (in coulombs) is a fully      charged 1.34-V zinc–mercuric oxide watch…

A: A cell consists of a single anode and a cathode isolated by an electrolyte used to create voltage…

Q: What happens to the chemical energy of a lithium-ion battery as it is discharged topower a laptop…

A: When the lithium ion battery is discharged to  power a laptop it would produces the electrical…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: Answer  = 3.50 grams

Q: Write each of the following in scientific notation, keeping the sig figs from the standard value: a.…

A: Scientific notation: Express any large or small value in the terms of a base of 10.

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: The electrochemical reaction of silver is –

Q: The gold plating of a ceramic figurine requires a total of 4.19 g of solid gold.  If the current…

A: Given  Mass of solid gold required = w = 4.19 g Current being used is = I = 11.0 amperes how many…

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the…

A: Given: Mass of god produced = 0.34 g. Current passed = 0.10 A

Q: A battery can provide a current of 3.40 A at 2.80 V for 8.50 hr. How much energy (in kJ) is…

A: The power of the battery is calculated as shown below. The power of the battery is 9.52 W or 9.52…

Q: Dlading When a lead acid car battery is recharged by the alternator, it acts essentially as an…

A: Current = 80.0A Time = 63.0 s

Q: A battery can provide a current of 3.80 A at 3.60 V for 8.00 hr. How much energy (in kJ) is…

A: Given that a current of 3.80 A was provided by battery at 3.60 V. The power can be calculated as…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: According to the Faraday's law of electrolysis, the mass of Substance liberated or deposited at any…

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: The balanced reaction taking place is given as, Given: Voltage = 10 V Current = 6.0 A And mass of…

Q: The oxidation of methanol, as described by the equation below, has a ΔG° value of -937.9 kJ/mol.…

A: Given Oxidation of Methanol 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)∆Gcell° = -937.9 kJ/mol =…

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.