Calculate Molar Mass Of Fluoxetine C17H18F3NO A Step-by-Step Guide

In chemistry, determining the molar mass of a compound is a fundamental skill. The molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). This value is crucial for various calculations, including converting between mass and moles, determining the stoichiometry of reactions, and preparing solutions of specific concentrations. In this comprehensive guide, we will walk through the step-by-step process of calculating the molar mass of Fluoxetine (C17H18F3NO), a widely used antidepressant medication. We will also delve into the importance of expressing the final answer to the correct number of significant figures and including the appropriate units. By understanding these concepts, you will be well-equipped to tackle similar calculations in your chemistry studies or professional endeavors.

Fluoxetine, with its chemical formula C17H18F3NO, presents an interesting case study due to the presence of multiple elements, each contributing to the overall molar mass of the compound. To accurately calculate the molar mass, we need to consider the atomic masses of each element present in the formula and the number of atoms of each element. This process involves referring to the periodic table for accurate atomic mass values and performing a simple calculation. The molar mass, expressed in grams per mole (g/mol), is a critical property for chemical calculations, especially when converting between mass and moles or determining reaction stoichiometry. This calculation provides a practical example of how the theoretical concepts of chemistry are applied in real-world scenarios, such as in pharmaceutical chemistry.

The significance of the molar mass calculation extends beyond academic exercises. In the pharmaceutical industry, accurate molar mass calculations are essential for drug formulation, dosage determination, and quality control. Fluoxetine, being a widely prescribed medication, requires precise calculations to ensure patient safety and efficacy. Understanding how to calculate the molar mass of Fluoxetine not only reinforces fundamental chemical principles but also highlights the practical relevance of chemistry in everyday life. This exercise emphasizes the importance of attention to detail, the correct use of the periodic table, and the application of mathematical skills in a chemical context.

To calculate the molar mass of Fluoxetine (C17H18F3NO), we need to break down the formula and consider the atomic mass of each element present. The chemical formula tells us that one molecule of Fluoxetine contains 17 carbon atoms (C), 18 hydrogen atoms (H), 3 fluorine atoms (F), 1 nitrogen atom (N), and 1 oxygen atom (O). The atomic masses of these elements can be found on the periodic table. Carbon has an atomic mass of approximately 12.01 g/mol, hydrogen is approximately 1.008 g/mol, fluorine is approximately 19.00 g/mol, nitrogen is approximately 14.01 g/mol, and oxygen is approximately 16.00 g/mol. These values are the foundation for our calculation and must be accurate to ensure the correct molar mass is determined.

Next, we multiply the atomic mass of each element by the number of atoms of that element in the formula. For carbon, we have 17 atoms, so we multiply 17 by 12.01 g/mol. For hydrogen, we have 18 atoms, so we multiply 18 by 1.008 g/mol. For fluorine, we have 3 atoms, so we multiply 3 by 19.00 g/mol. For nitrogen, we have 1 atom, so we multiply 1 by 14.01 g/mol. Finally, for oxygen, we have 1 atom, so we multiply 1 by 16.00 g/mol. These calculations give us the contribution of each element to the total molar mass of Fluoxetine. It is crucial to perform these multiplications accurately, paying attention to significant figures and units to maintain precision throughout the calculation.

After calculating the individual contributions of each element, we sum them up to obtain the total molar mass of Fluoxetine. This involves adding the results from the previous step: (17 * 12.01) + (18 * 1.008) + (3 * 19.00) + (1 * 14.01) + (1 * 16.00). Performing this addition carefully will give us the molar mass in grams per mole (g/mol). The result represents the mass of one mole of Fluoxetine molecules and is a fundamental property of the compound. This step requires careful attention to detail to ensure that all values are added correctly and that the final result is accurate. The sum represents the culmination of all the individual atomic mass contributions, providing a single value for the molar mass of Fluoxetine.

Let's perform the detailed calculation of the molar mass of Fluoxetine (C17H18F3NO), following the steps outlined earlier. First, we identify the atomic masses of each element: carbon (C) at 12.01 g/mol, hydrogen (H) at 1.008 g/mol, fluorine (F) at 19.00 g/mol, nitrogen (N) at 14.01 g/mol, and oxygen (O) at 16.00 g/mol. These values are obtained from the periodic table and are essential for accurate molar mass calculation. The precision of these atomic masses directly impacts the accuracy of the final result, highlighting the importance of using reliable sources for these values.

Next, we multiply each atomic mass by the number of atoms of that element in the Fluoxetine molecule:

• For carbon: 17 atoms * 12.01 g/mol = 204.17 g/mol
• For hydrogen: 18 atoms * 1.008 g/mol = 18.144 g/mol
• For fluorine: 3 atoms * 19.00 g/mol = 57.00 g/mol
• For nitrogen: 1 atom * 14.01 g/mol = 14.01 g/mol
• For oxygen: 1 atom * 16.00 g/mol = 16.00 g/mol

These calculations give us the individual mass contributions of each element in Fluoxetine. It's crucial to maintain the correct number of decimal places throughout these calculations to ensure accuracy in the final result. Each of these values represents the mass contributed by a specific element to the overall molar mass of the compound, providing a detailed breakdown of the molecular weight composition.

Finally, we add up all the individual contributions to find the total molar mass: 204.17 g/mol + 18.144 g/mol + 57.00 g/mol + 14.01 g/mol + 16.00 g/mol = 309.324 g/mol. This sum represents the molar mass of Fluoxetine, but we need to consider significant figures to provide the answer in the correct format. This final addition combines all the individual elemental contributions into a single value, representing the mass of one mole of Fluoxetine molecules. The result is a critical piece of information for various chemical calculations and applications.

In scientific calculations, significant figures are crucial for representing the precision of a measurement or calculation. When determining the molar mass of a compound, the number of significant figures in the atomic masses used will influence the number of significant figures in the final answer. In our calculation for Fluoxetine, we used atomic masses with varying numbers of significant figures. To maintain accuracy, we need to round our final answer to the least number of significant figures present in the initial values. The concept of significant figures ensures that our results accurately reflect the precision of the measurements and data used in the calculation.

Looking back at our atomic masses, fluorine (19.00 g/mol) has four significant figures, while the other elements also have at least four significant figures. Therefore, our final answer should be expressed to four significant figures. The calculated molar mass of Fluoxetine was 309.324 g/mol. Rounding this to four significant figures gives us 309.3 g/mol. This rounding step is essential to avoid overstating the precision of our result and to align the answer with the precision of the input values. The consideration of significant figures is a fundamental aspect of scientific calculations, ensuring that results are both accurate and appropriately represented.

Finally, it is essential to include the correct units with our answer. The molar mass is expressed in grams per mole (g/mol), which indicates the mass of one mole of the substance. Therefore, the molar mass of Fluoxetine, expressed to four significant figures with the correct units, is 309.3 g/mol. Including units in scientific calculations is not just a formality; it provides crucial context and meaning to the numerical value. The units clarify what the number represents and are essential for dimensional analysis and further calculations. The correct use of units is a hallmark of careful and accurate scientific work.

The molar mass of Fluoxetine (C17H18F3NO), calculated to four significant figures and including the appropriate units, is 309.3 g/mol. This result represents the mass of one mole of Fluoxetine and is essential for various chemical calculations and applications. The process of arriving at this answer involved several steps, including identifying the atomic masses of each element, multiplying each atomic mass by the number of atoms of that element in the molecule, summing the contributions of each element, and finally, rounding the result to the correct number of significant figures and including the appropriate units. Each step is crucial for ensuring the accuracy and correctness of the final result.

This calculation highlights the importance of understanding chemical formulas, atomic masses, and the concept of molar mass. The ability to accurately calculate molar mass is a fundamental skill in chemistry, necessary for converting between mass and moles, determining reaction stoichiometry, and preparing solutions of specific concentrations. Moreover, this example demonstrates the practical application of chemistry in areas such as pharmaceuticals, where precise calculations are essential for drug formulation and dosage determination. The molar mass of Fluoxetine is a critical parameter in pharmaceutical chemistry, influencing how the drug is used and administered.

In conclusion, the calculation of the molar mass of Fluoxetine serves as a valuable exercise in applying fundamental chemical principles. By carefully following the steps outlined, we have determined the molar mass to be 309.3 g/mol, expressed to four significant figures. This result not only provides a specific value for Fluoxetine but also reinforces the broader concepts of molar mass calculation, significant figures, and the importance of units in scientific measurements. This exercise underscores the interconnectedness of chemical concepts and their practical relevance in various fields.

The molar mass is a cornerstone concept in chemistry, serving as a bridge between the microscopic world of atoms and molecules and the macroscopic world of grams and kilograms that we can measure in the laboratory. Its significance spans across various areas of chemistry, making it an indispensable tool for chemical calculations and analyses. Understanding the molar mass and its applications is crucial for students and professionals alike, as it forms the basis for many other chemical concepts and calculations. The molar mass is not just a number; it’s a fundamental property that links the quantity of a substance to its mass.

One of the primary applications of molar mass is in converting between mass and moles. The mole is the SI unit for the amount of substance, and it represents Avogadro's number (6.022 x 10^23) of particles (atoms, molecules, ions, etc.). The molar mass provides the conversion factor between the mass of a substance (in grams) and the amount of the substance (in moles). This conversion is essential in stoichiometry, where we need to determine the amounts of reactants and products involved in a chemical reaction. Whether it's determining the limiting reactant or calculating the theoretical yield, the molar mass plays a pivotal role in these stoichiometric calculations. Accurate mass-to-mole conversions are crucial for precise experimental work and chemical synthesis.

Furthermore, molar mass is crucial in preparing solutions of specific concentrations. Molarity, defined as the number of moles of solute per liter of solution, is a common unit of concentration in chemistry. To prepare a solution of a specific molarity, we need to know the molar mass of the solute. This allows us to calculate the mass of solute needed to dissolve in a given volume of solvent to achieve the desired concentration. The accuracy of solution preparation directly depends on the correct use of molar mass in the calculations. This is particularly important in fields like analytical chemistry, biochemistry, and pharmaceuticals, where precise concentrations are critical for experimental results and product quality. In research and industrial settings, the ability to accurately prepare solutions is a fundamental skill underpinned by the concept of molar mass.