# Chemistry

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?

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.

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3. 👁 152
1. 136kg

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posted by Benny

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