The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C 14 H 18 N 2 O 5 . (d) How many hydrogen atoms are present in 1.00 mg of aspartame?

Hey everyone welcome back. So let's get started with this video. So here they want us to calculate the number of carbon atoms in 26. g of butane And we're told the mother mass of butane is 58. g per mole. Okay, so here we're told that there's 26.3 g of butane. Therefore that's going to be what we're going to start with. So it's going to be grams. Then from grams are going to want to go to moles And how are we going to get 2Molds? That is by using the molar mass of beauty in which we're actually told it's 58 .1 g per mole. Okay. And then for most we're going to want to find the moles of carbon in the formula of butane. Once again, we're going to look here and that's how we're going to find the moles of carbon. And then finally we're going to go to the number of carbon atoms. So Adams and we're going to go to their using avocados number Which is 6.02, 2 times 10 to the 23. Okay, so let's go ahead and start our store kilometer. So then we're going to start with the Graham's given, which is 26 0.3 grams of butane C four H 10. Okay, so here we're going to use the molar mass, which we're told is 58 .1g of beauty for one more C four H 10. Okay, so then for moles, we're going to find the moles of carbon. So then one more beauty. See for age 10 contains four moles of carbon. So four months. See, okay, finally we're going to go to atoms by using over gorgeous number. So then one more carbon is 6.0-2 Times 10 to the Adams of carbon. So then grams cancel out moles, cancel out moles of carbon cancel and we get Adams of carbon. We do the math and it's one 09 times 10 To the 24 atoms of carbon. Okay, thank you for watching. I hope this helped. And I'll see you in the next video.

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 40d

Chapter 3, Problem 40d

The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C₁₄H₁₈N₂O₅. (d) How many hydrogen atoms are present in 1.00 mg of aspartame?

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Determine the molar mass of aspartame (C_{14}H_{18}N_{2}O_{5}) by adding the atomic masses of all the atoms in the formula.

Convert the mass of aspartame from milligrams to grams, since molar mass is typically in grams per mole.

Calculate the number of moles of aspartame using the formula: \( \text{moles} = \frac{\text{mass in grams}}{\text{molar mass}} \).

Use Avogadro's number (6.022 \times 10^{23} molecules/mol) to find the number of molecules of aspartame in the calculated moles.

Multiply the number of molecules of aspartame by the number of hydrogen atoms per molecule (18) to find the total number of hydrogen atoms.

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Key Concepts

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

Molecular Formula

A molecular formula indicates the number and types of atoms in a molecule. For aspartame, C14H18N2O5 means it contains 14 carbon atoms, 18 hydrogen atoms, 2 nitrogen atoms, and 5 oxygen atoms. Understanding the molecular formula is essential for determining the composition of a compound and calculating quantities such as mass or number of atoms.

Molar Mass

The molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the number of hydrogen atoms in a given mass of aspartame, one must first calculate its molar mass by summing the atomic masses of all atoms in the molecular formula. This allows for conversions between mass and the number of molecules or atoms.

Avogadro's Number

Avogadro's number, approximately 6.022 x 10^23, is the number of particles (atoms, molecules, etc.) in one mole of a substance. This concept is crucial for converting between moles and the actual number of molecules or atoms. In the context of aspartame, it helps determine how many hydrogen atoms are present in a specific mass of the compound by relating moles to individual atoms.