Posted by **Chemistry** on Friday, April 13, 2007 at 3:57pm.

A certain mine produces 2.5 108 kg of copper from chalcopyrite (CuFeS2) each year. The ore contains only 0.80% Cu by mass.

(a) If the density of the ore is 2.0 g/cm3, calculate the volume of ore removed each year.

(b) Calculate the mass of SO2 produced by roasting (assume chalcopyrite to be the only source of sulfur).

I don't even know where to begin.

For a, 0.8% of some mass (say x) = 2.5108 kg. Calculate x = mass ore that must be mined to obtain 2.5 kg Cu.

Change that to grams, then mass = volume x density. You know mass and density; calculatr volume. Part b is a stoichiometry problem. Write the equation, balance it, convert g Cu to mols, convert mols Cu to mols SO2, convert mols SO2 to grams. Post any work if you need futher assistance.