# Carbonate rocks like limestone (CaCO3) react with dilute acids such as HCl to produce carbon dioxide. [Solved] 14.8g
7.55L

molar mass of limestone = 40 12 3(16) = 100 g
Added the relative atomic masses of the atoms in CaCO3
fraction of a mole in 33.7 g of CaCO3 = 33.7/100 = 0.337

from the equation 1 mole of CO2 comes from 1mole of CaCO3.
So we now calculate the mass of 1 mole of CO2
adding the masses of CO2 = 12 2(16) = 12 32 = 44g
so mass of CO2 formed = 0.337 x 44 = 14.28g

at room temperature and pressure 1 mole of any gas has a volume 24 litres
So 0.337 moles of CO2 has volume = 0.337 x 24=8.088 litre
at room temperature and pressure.Some times the volume is asked for at normal temperature and pressure.The volume of a mole of any gas at ntp = 22.4 litres;so you could recalculate your gas volume at ntp as an exercise if you want the practice.

14.8g
7.55L

14.8g
7.55L

This post is last updated on hrtanswers.com at Date : 1st of September – 2022

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