posted by Ally on .
I was wondering if you could help me with this problem.
If the reaction proceeds with a 96.8% yield, how many kilograms of CaSO4 are formed when 5.34 kg SO2 reacts with an exfess of CaCO3 and O2?
Thanks for your help.
Write the equation for the reaction and balance it.
CaCO3 + SO2 ==> CaSO4 + ??
Change 5.34 kg SO2 to grams.
Change grams SO2 to mols. # mols = grams/molar mass SO2.
There is 1 mol SO2 in a mol of CaSO4; therefore, there will be the same number of mols formed of CaSO4 that you have of SO2 initially (at 100% yield).
Change mols CaSO4 to grams using mols = g/molar mass.
Change grams CaSO4 to kg.
kg CaSO4 @ 96.8% yield = kg CaSO4 @ 100% yield x 0.968.
Post your work if you get stuck.