Solid calcium carbonate (CaCO3) reacts with hydrochloric acid (HCI) to form carbon dioxide, water, and

calcium chloride (CaCl), according to this equation:

CaCO3 (s) + 2HCl (aq) - CaCl2 (aq) + H2O (aq) + CO2 (g)

Which of these actions would increase the rate of this reaction? Check all that apply.

using a more concentrated HCl solution

crushing the CaCO3 into a fine powder

increasing the pressure on the system

Using a more concentrated HCl solution and Crushing the CaCO₃ into a fine powder makes the reaction to occur at a faster rate.

Explanation:

CaCO₃ (s) + 2HCl (aq) → CaCl₂ (aq) + H₂O (aq) + CO₂ (g)

When calcium carbonate reacts with hydrochloric acid, it gives out carbon-dioxide in the form of bubbles and there is a formation of calcium chloride in aqueous medium.

The rate of the reaction can be increased by

Using a more concentrated HCl solution Crushing the CaCO₃ into a fine powder

When concentrated acid is used instead of dilute acid then the reaction will occur at a faster rate.

When CaCO₃ is crushed into a fine powder then the surface area will increases thereby increasing the rate of the reaction.

Answer: 1 & 2