# calculate the mass of sulphuric acid required to decompose 25g of pure marble. what is the volume of the Co2 if measured at STP

CaCO

_{3}(s) + H

_{2}SO

_{4}(aq) $\to $ CaSO

_{4}(aq) + CO

_{2}+ H

_{2}O

1 mole of pure marble reacts with 1 mole of sulphuric acid to give 1 mole of carbon dioxide.

2. Mass of Sulphuric Acid:

Number of moles of Calcium Carbonate = $\frac{Givenmass}{Molarmass}=\frac{25}{100}=\frac{1}{4}$

Mass of Sulphuric acid = $\frac{1}{4}\times 98=24.5g$

3. Volume of Carbon dioxide:

1 mole of gas at STP has volume 22.4 L

So, Volume of Carbon dioxide = $\frac{1}{4}\times 22.4=5.6L$

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