In the electrolysis of water, how many coulombs of charge are needed to produce 1.00 L of oxygen at 25.0 °C and 1.00 atm pressure? (F = 96500 C/mol)

A lead storage battery delivers a current of 6.00 A for one hour and 22 minutes at a voltage of 12.0 V. (a) How many grams of lead are converted to PbSO4? (b) How much electrical energy is produced in kilowatt hours?

Calcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?

A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?

Calculate the maximum work available from 50.0 g of aluminum in the following cell when the cell potential is 1.15 V. Al(s)Al3+(aq)H+(aq)O2(g)Pt Note that O2 is reduced to H2O.

A fuel cell designed to react grain alcohol with oxygen has the following net reaction: C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) The maximum work that 1 mole of alcohol can do is 1.32 103 kJ. What is the theoretical maximum voltage this cell can achieve at 25C?

When molten lithium chloride, LiCl, is electrolyzed, lithium metal is liberated at the cathode. How many grams of lithium are liberated when 2.00 103 C of charge passes through the cell?

An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?

Copper can be plated onto a spoon by placing the spoon in an acidic solution of CuSO4(aq) and connecting it m a copper strip via a power source as illustrated below: a. Label the anode and cathode. and describe the direction of the electron now. b. Write out the chemical equations for the reactions that occur at each electrode.

The commercial production of magnesium is accomplished by electrolysis of molten MgCl2. (a) Why is electrolysis of an aqueous solution of MgCl2 not used in this process? (b) Write the anode and cathode half-reaction in the electrolysis of molten MgCl2.