Calculate The Percentage Composition Of Nh4 2co3

Calculating the Percentage Composition of (NH₄)₂CO₃: A Step-by-Step Guide

Ammonium carbonate, (NH₄)₂CO₃, is an inorganic salt with a wide range of applications, from baking and medicine to fire extinguishing and fertilizer production. Understanding its percentage composition is crucial in various chemical calculations and applications. This comprehensive guide will walk you through the process of calculating the percentage composition of each element in ammonium carbonate step-by-step, providing a clear and detailed explanation along the way.

Understanding Percentage Composition

Percentage composition in chemistry refers to the relative mass percentage of each element present in a compound. It indicates the proportion of each element that contributes to the overall mass of the compound. This information is essential for various reasons, including:

Stoichiometric calculations: Determining the amount of reactants needed in a chemical reaction.
Empirical formula determination: Finding the simplest whole-number ratio of atoms in a compound.
Purity analysis: Assessing the purity of a chemical sample.
Understanding chemical properties: Relating the composition of a compound to its observed properties.

Calculating percentage composition involves determining the molar mass of each element in the compound and comparing it to the molar mass of the entire compound.

Calculating the Molar Mass of (NH₄)₂CO₃

Before we can calculate the percentage composition, we need to determine the molar mass of ammonium carbonate, (NH₄)₂CO₃. This is done by summing up the atomic masses of all the atoms present in one mole of the compound.

We'll use the following standard atomic masses:

N (Nitrogen): 14.01 g/mol
H (Hydrogen): 1.01 g/mol
C (Carbon): 12.01 g/mol
O (Oxygen): 16.00 g/mol

Let's break down the calculation:

Nitrogen (N): 2 N atoms × 14.01 g/mol/N atom = 28.02 g/mol
Hydrogen (H): 8 H atoms × 1.01 g/mol/H atom = 8.08 g/mol
Carbon (C): 1 C atom × 12.01 g/mol/C atom = 12.01 g/mol
Oxygen (O): 3 O atoms × 16.00 g/mol/O atom = 48.00 g/mol

Total molar mass of (NH₄)₂CO₃ = 28.02 g/mol + 8.08 g/mol + 12.01 g/mol + 48.00 g/mol = 96.11 g/mol

Calculating the Percentage Composition of Each Element

Now that we have the molar mass of (NH₄)₂CO₃, we can calculate the percentage composition of each element. The formula for percentage composition is:

(Mass of element / Molar mass of compound) × 100%

Let's apply this formula to each element in ammonium carbonate:

Percentage Composition of Nitrogen (N)

Mass of Nitrogen in (NH₄)₂CO₃ = 28.02 g/mol
Percentage of Nitrogen = (28.02 g/mol / 96.11 g/mol) × 100% = 29.15%

Percentage Composition of Hydrogen (H)

Mass of Hydrogen in (NH₄)₂CO₃ = 8.08 g/mol
Percentage of Hydrogen = (8.08 g/mol / 96.11 g/mol) × 100% = 8.41%

Percentage Composition of Carbon (C)

Mass of Carbon in (NH₄)₂CO₃ = 12.01 g/mol
Percentage of Carbon = (12.01 g/mol / 96.11 g/mol) × 100% = 12.50%

Percentage Composition of Oxygen (O)

Mass of Oxygen in (NH₄)₂CO₃ = 48.00 g/mol
Percentage of Oxygen = (48.00 g/mol / 96.11 g/mol) × 100% = 49.94%

Verification of Results

To ensure the accuracy of our calculations, we can check if the sum of the individual percentage compositions adds up to approximately 100%. Minor discrepancies might arise due to rounding errors.

29.15% + 8.41% + 12.50% + 49.94% = 100.00%

The sum is exactly 100%, confirming the accuracy of our calculations.

Practical Applications of Percentage Composition

The percentage composition of (NH₄)₂CO₃ has several practical applications:

Fertilizer industry: Knowing the nitrogen content (29.15%) is crucial for determining the appropriate amount of ammonium carbonate needed to provide a specific nitrogen dose to plants.
Baking: In baking, ammonium carbonate acts as a leavening agent. Understanding its composition helps bakers control the amount of gas produced during baking.
Chemical analysis: Percentage composition is essential in determining the purity of a sample of ammonium carbonate.
Pharmaceutical applications: Ammonium carbonate is used in some medications; precise composition is vital for dosage control.
Fire extinguishing: The composition informs the efficiency of ammonium carbonate in firefighting applications.

Conclusion: Mastering Percentage Composition Calculations

Calculating the percentage composition of chemical compounds is a fundamental skill in chemistry. This detailed guide demonstrated the step-by-step process of calculating the percentage composition of ammonium carbonate, (NH₄)₂CO₃. By understanding this process, you can confidently tackle similar calculations for other compounds and apply this knowledge to various chemical applications and analyses. Remember to always double-check your calculations and ensure the sum of the percentages is close to 100%. This will help you build confidence in your results and solidify your understanding of this important chemical concept. Understanding percentage composition lays the groundwork for more advanced chemical concepts and calculations, making it a crucial skill to master for anyone interested in chemistry.