Question

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

Answer 1

Answer: 1 & 2

Step-by-step explanation:

Answer 2

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

Step-by-step 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.