An electric current of 1.04 A was passed through a solution of dilute sulfuric acid for 6.00 min. The volume of hydrogen produced at r.t.p. was 43.5 cm³.

a. How many coulombs of charge were passed during the experiment?

b. How many coulombs of charge are required to liberate 1 mole of hydrogen gas?  (F = 96 500 C mol^–1)

c. In another experiment, copper(II) sulfate was electrolysed using copper electrodes. Copper was deposited at the cathode.

i. Write a half-equation for this reaction.

ii. A student conducted an experiment to calculate a value for the Faraday constant, F. An electric current of 0.300 A was passed through the solution of copper(II) sulfate for exactly 40 min. 0.240 g of copper was deposited at the cathode. Use this information to calculate a value for F. Express your answer to 3 significant figures. (A_r value: [Cu] = 63.5)

iii. The charge on one electron is approximately 1.60 × 10^–19 C. Use this information and your answer to part ii to calculate a value for the Avogadro constant.