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

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.

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we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).