Decomposing Calcium Carbonate with 60% Sulfuric Acid: An In-Depth Analysis
Decomposing Calcium Carbonate with 60% Sulfuric Acid: An In-Depth Analysis
Decomposing raw materials with sulfuric acid is a common practice in various industrial and chemical processes. In this article, we will delve into the chemical reaction required to decompose 25 grams of calcium carbonate (CaCO?) with 60% sulfuric acid (H?SO?). This process not only aids in understanding the underlying chemistry but also has practical applications in industries such as manufacturing and environmental management.
Chemical Reaction Involved
The reaction between calcium carbonate and sulfuric acid is a classic example of a chemical decomposition reaction. It can be represented by the following balanced equation:
CaCO? H?SO? → CaSO? H?O CO?
Step-by-Step Calculation
Step 1: Calculate Moles of CaCO?
First, we need to determine the moles of calcium carbonate in 25 grams. The molar mass of calcium carbonate (CaCO?) is calculated as follows:
Molar mass of CaCO? Ca (40.08 g/mol) C (12.01 g/mol) 3O (16.00 g/mol × 3)
40.08 12.01 48.00 100.09 g/mol
Using the formula:
Moles of CaCO? Mass / Molar Mass 25 g / 100.09 g/mol ≈ 0.2498 mol
Step 2: Calculate Moles of H?SO? Required
From the balanced equation, it is clear that one mole of CaCO? reacts with one mole of H?SO?. Therefore, the moles of H?SO? required to decompose 25 grams of CaCO? are also approximately 0.2498 moles.
Step 3: Calculate Mass of H?SO? Required
The molar mass of sulfuric acid (H?SO?) is calculated as:
Molar mass of H?SO? 2H (1.01 g/mol × 2) S (32.07 g/mol) 4O (16.00 g/mol × 4)
2.02 32.07 64.00 98.09 g/mol
Using the calculated moles and molar mass, the mass of H?SO? required can be calculated as:
Mass of H?SO? Moles × Molar Mass 0.2498 mol × 98.09 g/mol ≈ 24.5 g
Step 4: Calculate the Mass of 60% Pure H?SO? Needed
Since the sulfuric acid is 60% pure, the total mass of the pure solution needed is:
Mass of 60% H?SO? Mass of pure H?SO? / Purity 24.5 g / 0.60 ≈ 40.83 g
Practical Applications
Understanding the specific requirements for chemical reactions like the decomposition of calcium carbonate can be crucial for industries. For instance, in environmental management, this knowledge can be used in neutralizing acidic soils or in wastewater treatment. In manufacturing processes, precise calculations like these ensure efficient and safe chemical reactions.
To further understand the amount required, we can calculate the volume of 60% pure sulfuric acid:
Volume of 60% H?SO? Mass of solution / Density 40.83 g / 1.4983 g/mL ≈ 27.25 mL
Summary
To decompose 25 grams of chalk (CaCO?) with 60% pure sulfuric acid (H?SO?), approximately 40.83 grams of 60% pure sulfuric acid is required. This process involves calculating moles and masses based on the balanced chemical equation, ensuring precise and efficient chemical reactions. Understanding these calculations can help in various industrial and environmental applications.