[Borek]

Mixture of CaO and CaCO₃ was reacted stoichiometrically with a solution of hydrochloric acid, producing 8.04 L of CO₂ (measured at 290 K and 120 kPa). Mass of the dry CaCl₂ obtained was 50.61% higher than the mass of the original mixture. How much water was present in the 1M HCl solution used for the reaction, if its density was 1.02 g/mL?

[XGen]

1.95 kg?

[Bublik]

I get 1.91L :S

[curiouscat]

1965 gm?

PS. Why do we not consider this reaction:

CaO + H2O  Ca(OH)₂

Does it not occur? Or will HCl ultimately convert Ca(OH)2 to CaCl₂?

[Borek]

1965 gm?

This is closest to the number I was looking for. I got 1967 g. Could be the difference is in the molar masses, I am using EBAS which means I am using exact numbers, not approximate ones.

PS. Why do we not consider this reaction:

CaO + H2O  Ca(OH)₂

Does it not occur? Or will HCl ultimately convert Ca(OH)2 to CaCl₂?

Yes, even if CaO reacts with water, later water is regenerated in the reaction of hydroxide with HCl. We are told amount of acid was stoichiometric.

[Rutherford]

I got that result when I used that the number of moles are 0.4 and 0.6mol (for the salts) n of HCl is therefore 2mol, and that the mass share is 3.5784% (4 digits). So:
73g:x=3.5784%:(100-3.5784)%, x=1967.02g of water.