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Chapter 20: Problem 19

One harmful effect of acid rain is the deterioration of structures and statues made of marble or limestone, both of which are essentially calcium carbonate. The reaction of calcium carbonate with sulfuric acid yields carbon dioxide, water, and calcium sulfate. Because calcium sulfate is marginally soluble in water, part of the object is washed away by the rain. Write a balanced chemical equation for the reaction of sulfuric acid with calcium carbonate.

Short Answer

Expert verified
The balanced chemical equation for the reaction of sulfuric acid (H鈧係O鈧�) with calcium carbonate (CaCO鈧�) is: \( \text{H}_2\text{SO}_4 + \text{CaCO}_3 \rightarrow \text{CO}_2 + \text{H}_2\text{O}+ \text{CaSO}_4 \).

Step by step solution

01

Identify the Reactants and Products

The given reactants are sulfuric acid (H鈧係O鈧�) and calcium carbonate (CaCO鈧�). When these react, they produce carbon dioxide (CO鈧�), water (H鈧侽), and calcium sulfate (CaSO鈧�).
02

Write an Unbalanced Chemical Equation

Having the formulae of the reactants and the products, we write them in the correct order of a chemical equation. Reactants are always on the left (LHS) and the products on the right (RHS): \( \text{H}_2\text{SO}_4 + \text{CaCO}_3 \rightarrow \text{CO}_2 + \text{H}_2\text{O}+ \text{CaSO}_4 \)
03

Balance the Chemical Equation

On first look, there are 2 oxygen atoms on LHS in the compound CaCO鈧� and 5 on the RHS. To balance the equation, we need to make sure the numbers of each type of atom on both sides of the equation are equal. The easiest way to do this is to adjust the coefficients (the numbers in front of atoms or compounds). First, balance the calcium atoms by putting a 1 in front of CaCO鈧� and CaSO鈧�. Next, balance the sulfur atoms by also putting a 1 in front of H鈧係O鈧� and CaSO鈧�. For the carbon atoms, put a 1 in front of CaCO鈧� and CO鈧�. To balance the hydrogen and oxygen atoms, put a 2 in front of H鈧侽. Now, recheck the balance of the oxygen atoms. If it is not balanced, adjust the number appropriately. After balancing atoms of each element, the balanced equation is: \( \text{H}_2\text{SO}_4 + \text{CaCO}_3 \rightarrow \text{CO}_2 + \text{H}_2\text{O}+ \text{CaSO}_4 \) This means that one molecule of sulfuric acid reacts with one molecule of calcium carbonate to produce one molecule of carbon dioxide, one molecule of water and one molecule of calcium sulfate. Since no other adjustments are needed, this is the balanced equation for the reaction.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Equation Balancing
Chemical equation balancing is a fundamental aspect of chemistry that ensures the isotopic and mass matters are equivalent on both sides of a reaction. When we balance a chemical equation, we adjust the number of units鈥攃alled "coefficients"鈥攖o ensure the same number of every type of atom appears on both sides of the equation.
For the reaction between sulfuric acid and calcium carbonate, the initial unbalanced equation is \( \text{H}_2\text{SO}_4 + \text{CaCO}_3 \rightarrow \text{CO}_2 + \text{H}_2\text{O} + \text{CaSO}_4 \). This equation is balanced when the coefficients are correctly determined.
This balance ensures that there are equal numbers of calcium, sulfur, carbon, hydrogen, and oxygen atoms on each side of the equation, following the law of conservation of mass. Balancing chemical equations is not only a good practice for standardized reactions; it also helps chemists understand the proportions necessary for various chemical reactions in practice.
Sulfuric Acid
Sulfuric acid (H鈧係O鈧�) is a highly corrosive, strong mineral acid that is a major component of acid rain. It is among the most important compounds in industrial chemistry.
In the reaction we're discussing, sulfuric acid reacts with calcium carbonate found in building materials like marble and limestone. This reaction contributes to the deterioration of historic structures, as the acid slowly erodes these materials.
The notable properties of sulfuric acid include:
  • A strong acidic nature, capable of dissolving metals and minerals.
  • High affinity for water, creating extremely exothermic hydration processes.
  • Its ability to donate protons (H鈦� ions), which simplifies replacement in ionic compounds.
These characteristics make sulfuric acid a useful but potentially dangerous substance when used improperly.
Calcium Carbonate
Calcium carbonate (CaCO鈧�) is a common substance found in rocks as minerals such as limestone and marble. Structures made of these materials are susceptible to damage from acid rain due to their reaction with sulfuric acid.
When sulfuric acid reacts with calcium carbonate, it forms calcium sulfate (CaSO鈧�), carbon dioxide (CO鈧�), and water (H鈧侽). This process not only alters the carbonate but also contributes to the gradual erosion of stone monuments.
Key points about calcium carbonate:
  • It is insoluble in water but interacts readily with acids.
  • Widely used in construction, it forms the basic component of cement and lime.
  • The reaction with acids is an example of acid-base reaction.
This illustrates the dual role of calcium carbonate both as an architectural cornerstone and a chemical that can be transformed easily under acid-mediated conditions.
Reaction Products
The reaction between sulfuric acid and calcium carbonate yields several important products. These products are carbon dioxide, water, and calcium sulfate.
  • Carbon Dioxide (CO鈧�): A gas that is a major product of this reaction, it is released into the atmosphere, contributing to natural carbon cycles.
  • Water (H鈧侽): Formed as a byproduct, water accompanies other products and potentially aids in the transportation of dissolved substances away from structures.
  • Calcium Sulfate (CaSO鈧�): Also known as gypsum in its hydrated form, this is less durable than calcium carbonate and can be washed away over time, leading to structural erosion.
This decomposition of calcium carbonate not only explains the visible effects of acid rain on stone structures but also highlights the critical interaction between environmental chemistry and physical architecture.

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Most popular questions from this chapter

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