(a) Ibuprofen is a common over-the-counter analgesic with the formula C 13 H 18 O 2 . How many moles of C 13 H 18 O 2 are in a 500-mg tablet of ibuprofen? Assume the tablet is composed entirely of ibuprofen.

Hi everyone here we have a question telling us that an alternative sweetener stevia has a molecular formula of C. 54 age 70 oh 23. And our goal is to calculate the malls of stevia in 5.0 mg of this substance. So first we need to calculate the molar mass of stevia. So we have carbon and we have 44 of them. And if we look on the periodic table we see that smaller masses 12.01, which equals 528.44. And then we have hydrogen. We have 70 of them times 1. equals 70.7. And then we have oxygen. We have 23 of them And it's more masses 16. That equals 368. For a total of 967. g per mole. So we have 5.00 mg of stevia. And we first need to change that into g. So we're gonna multiply by 10 to the negative 3rd g Divided by one mg times one more Divided by its Molar mass 967. g. And our milligrams are going to cancel out our grams are gonna cancel out, leading us with 5.17 times 10 to the negative six g. And that is our final answer. Thank you for watching. Bye

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 90a

Chapter 3, Problem 90a

(a) Ibuprofen is a common over-the-counter analgesic with the formula C₁₃H₁₈O₂. How many moles of C₁₃H₁₈O₂are in a 500-mg tablet of ibuprofen? Assume the tablet is composed entirely of ibuprofen.

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First, determine the molar mass of ibuprofen (C13H18O2) by adding the atomic masses of all the atoms in the formula. Use the periodic table to find the atomic masses: Carbon (C) is approximately 12.01 g/mol, Hydrogen (H) is approximately 1.01 g/mol, and Oxygen (O) is approximately 16.00 g/mol.

Calculate the molar mass of ibuprofen by multiplying the number of each type of atom by its atomic mass and then summing these values: (13 * 12.01 g/mol) + (18 * 1.01 g/mol) + (2 * 16.00 g/mol).

Convert the mass of the ibuprofen tablet from milligrams to grams, since molar mass is in grams per mole. Remember that 1 gram = 1000 milligrams, so divide 500 mg by 1000 to convert to grams.

Use the formula for moles, which is: moles = mass (in grams) / molar mass (in g/mol). Substitute the mass of the ibuprofen tablet in grams and the molar mass of ibuprofen into this formula.

Perform the division to find the number of moles of ibuprofen in the 500-mg tablet. This will give you the final answer in moles.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a chemical formula. For ibuprofen (C13H18O2), the molar mass can be determined by adding the masses of 13 carbon (C), 18 hydrogen (H), and 2 oxygen (O) atoms, which is essential for converting between grams and moles.

Conversion from Mass to Moles

To find the number of moles from a given mass, the formula used is: moles = mass (g) / molar mass (g/mol). This relationship allows us to convert the mass of a substance into the number of moles, which is a fundamental concept in stoichiometry. In this case, we will convert the mass of the ibuprofen tablet (500 mg) into grams before applying this formula.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It involves using balanced chemical equations to calculate the amounts of substances involved. In this question, stoichiometry is applied to determine how many moles of ibuprofen are present in a specific mass of the compound, which is crucial for understanding dosage and pharmacology.

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Textbook Question

Very small semiconductor crystals, composed of approximately 1000 to 10,000 atoms, are called quantum dots. Quantum dots made of the semiconductor CdSe are now being used in electronic reader and tablet displays because they emit light efficiently and in multiple colors, depending on dot size. The density of CdSe is 5.82 g/cm³. (c) What is the mass of one 6.5-nm CdSe quantum dot?

(a) Ibuprofen is a common over-the-counter analgesic with the formula C13H18O2. How many moles of C13H18O2 are in a 500-mg tablet of ibuprofen? Assume the tablet is composed entirely of ibuprofen.

Verified video answer for a similar problem:

Key Concepts

Molar Mass

Conversion from Mass to Moles

Stoichiometry

(a) Ibuprofen is a common over-the-counter analgesic with the formula C₁₃H₁₈O₂. How many moles of C₁₃H₁₈O₂are in a 500-mg tablet of ibuprofen? Assume the tablet is composed entirely of ibuprofen.