Question

The mass of \[C{O_2}\] obtained when \[60g\] of calcium carbonate is treated with excess of hydrochloric acid:
a) $30.0g$
b) $15.0g$
C) $13.2g$
d) $26.4g$

Answer 1

Hint: We know that $CaC{O_3}$ is a substance found in rocks as the minerals calcite and aragonite (most remarkably as limestone, which is a kind of sedimentary stone comprising predominantly of calcite) and is the fundamental part of eggshells, snail shells, shells and pearls. It is the dynamic fixing in horticultural lime and is made when calcium particles in hard water respond with carbonate particles to make limescale. It has clinical use as a calcium supplement or as an acid neutralizer, however inordinate utilization can be perilous and cause hypocalcaemia and stomach related problems.

Complete answer:
The balanced equation is,
\[CaC{O_3}\left( s \right) + 2HCl\left( {aq} \right) \to CaC{l_2}\left( {aq} \right){\text{ + }}C{O_2}\left( g \right) + {H_2}O\left( l \right)\]
From the balanced equation it is known that one mole of calcium carbonate produces one mole of carbon dioxide.
We know that the molecular weight of calcium carbonate is \[100g/mol\]
\[60gCaC{O_3} = 60g/100g/mol = 0.60mol\]
Thus, the number of carbon dioxide produced is $0.60mol$
We know that the Molar mass of carbon dioxide is \[44g/mol\]
The Mass of carbon dioxide produced is calculated as,
\[Mass = 0.60mol \times 44g/mol = 26.4gC{O_2}produced\]

Hence option d is correct.

Note:
Calcium carbonate shares the average properties of different carbonates. Prominently it
Responds with acids, delivering carbon dioxide in fact talking, carbonic corrosive, yet that crumbles rapidly to Carbon dioxide and water:
\[CaC{O_3}\left( s \right) + 2{H^ + }\left( {aq} \right) \to C{a^{2 + }}\left( {aq} \right) + C{O_2}\left( g \right) + {H_2}O\left( l \right)\]
Discharges carbon dioxide after warming, called a warm disintegration response, or calcination (to over \[840^\circ C\] on account of \[CaC{O_3}\] ), to shape calcium oxide, generally called quicklime, with response enthalpy \[178{\text{ }}kJ/mol\]:
\[CaC{O_3}\left( s \right) \to CaO\left( s \right) + C{O_2}\left( g \right)\]
Calcium carbonate will respond with water that is immersed with carbon dioxide to shape the solvent calcium bicarbonate.
\[CaC{O_3}\left( s \right) + C{O_2}\left( g \right) + {H_2}O\left( l \right) \to Ca{\left( {HC{O_3}} \right)_2}\left( {aq} \right)\]
This response is significant in the disintegration of carbonate rock, framing natural hollows, and prompts hard water in numerous locales. A strange type of calcium carbonate is the hexahydrate,\[CaC{O_3}\cdot6{H_2}O\] and it is steady just under \[8^\circ C\].