when marble undergoes CaCO3+ H2SO4 = CaSO4+H2O+CO2, what happens to it and where can one see the evidence of this effect?

When marble (calcium carbonate, CaCO3) reacts with sulfuric acid (H2SO4), a chemical reaction takes place. Here is the balanced equation for the reaction:

CaCO3 + H2SO4 → CaSO4 + H2O + CO2

During this reaction, calcium carbonate reacts with sulfuric acid to produce calcium sulfate, water, and carbon dioxide.

Now, let's discuss what happens to the marble and where one can observe evidence of this reaction:

1. Dissolution of Marble: As the sulfuric acid comes into contact with the marble, it reacts with the calcium carbonate present in the marble. This reaction causes the marble to dissolve as the solid calcium carbonate is converted into soluble calcium sulfate.

2. Formation of Calcium Sulfate: The calcium carbonate reacts with sulfuric acid, resulting in the formation of calcium sulfate (CaSO4). Calcium sulfate is a white solid that can be observed as a residue or precipitate during the reaction. This solid may appear as visible deposits or a layer on the surface of the marble.

3. Release of Carbon Dioxide: One of the products of the reaction is carbon dioxide (CO2). Carbon dioxide is a gas and as it is liberated, bubbles may form in the liquid, or if the reaction is happening on a solid surface, gas production can result in effervescence or fizzing. This is one of the most noticeable effects of the reaction.

4. Formation of Water: Another product of the reaction is water (H2O). Since water is a liquid, it may not be readily observable during the reaction unless it accumulates in a noticeable amount.

To observe the evidence of this effect, one can carry out the reaction experimentally. By mixing marble chips or powdered marble (calcium carbonate) with sulfuric acid, you can visually see the marble dissolving, the formation of white calcium sulfate residue, and the release of carbon dioxide gas. It is important to note that this reaction should be performed with caution and under appropriate laboratory conditions due to the use of sulfuric acid, which is a strong and corrosive acid.