How many bromine atoms are present in 35.2 g of CH 2 Br 2 ?

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 - Molecules, Compounds & Chemical Equations

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Ch.3 - Molecules, Compounds & Chemical Equations

Problem 86

Chapter 3, Problem 86

How many bromine atoms are present in 35.2 g of CH₂Br₂?

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Calculate the molar mass of CH2Br2 by adding the atomic masses of all the atoms in the compound: C (12.01 g/mol), H (1.01 g/mol each), and Br (79.90 g/mol each).

Determine the number of moles of CH2Br2 in 35.2 g by using the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Recognize that each molecule of CH2Br2 contains 2 bromine atoms.

Calculate the total number of bromine atoms by multiplying the number of moles of CH2Br2 by Avogadro's number (\(6.022 \times 10^{23}\) molecules/mol) and then by 2 (since there are 2 Br atoms per molecule).

Express the final result as the total number of bromine atoms present in the given mass of CH2Br2.

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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 the atoms in a molecule. For CH2Br2, the molar mass can be determined by adding the masses of carbon (C), hydrogen (H), and bromine (Br) atoms, which is essential for converting grams of the compound to moles.

Avogadro's Number

Avogadro's number, approximately 6.022 x 10^23, is the number of atoms, ions, or molecules in one mole of a substance. This constant allows chemists to relate the mass of a substance to the number of particles it contains. In this context, it will be used to determine how many bromine atoms are present in the moles of CH2Br2 calculated from the given mass.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows for the calculation of the amount of substances involved based on their molar ratios. In this case, stoichiometry will help determine the number of bromine atoms in the given mass of CH2Br2 by using the mole ratio from the molecular formula.

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How many bromine atoms are present in 35.2 g of CH2Br2?

Verified video answer for a similar problem:

Key Concepts

Molar Mass

Avogadro's Number

Stoichiometry

How many bromine atoms are present in 35.2 g of CH₂Br₂?