(a) Write a chemical equation that describes the attack of acid rain on limestone, \(\mathrm{CaCO}_{3}\). (b) If a limestone sculpture were treated to form a surface layer of calcium sulfate, would this help to slow down the effects of acid rain? Explain.

Acid rain is caused mainly due to the emission of sulfur dioxide (SO2) and nitrogen oxides (NOx) from industries and automobiles. In the atmosphere, these gases react with water vapor to form sulfuric acid (H2SO4) and nitric acid (HNO3), which fall back to the earth's surface as acid rain.

Here, we will focus on the reaction of sulfuric acid (H2SO4) with limestone (CaCO3). When sulfuric acid comes into contact with limestone, it reacts to form calcium sulfate, carbon dioxide, and water. The balanced chemical equation for this reaction is: \[CaCO_{3}(s) + H_{2}SO_{4}(aq) \rightarrow CaSO_{4}(s) + CO_{2}(g) + H_{2}O(l)\]

Now we need to examine if treating limestone sculptures with a surface layer of calcium sulfate would help slow down the effects of acid rain. Calcium sulfate is more resistant to acid rain attack as compared to calcium carbonate. Treating the surface of limestone sculptures with calcium sulfate will create a barrier between the limestone and the acid rain, preventing the direct contact of acid with the limestone CaCO3. Since calcium sulfate is relatively insoluble in water and doesn't react with acid rain like limestone, it will help slow down the decay of the limestone sculpture caused by acid rain. So, the answer to part (b) is yes, treating the limestone sculpture to form a surface layer of calcium sulfate would help slow down the effects of acid rain.