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Chapter 3: Problem 52

The Freons are a class of compounds containing carbon, chlorine, and fluorine. While they have many valuable uses, they have been shown to be responsible for depletion of the ozone in the upper atmosphere. In 1991 , two replacement compounds for Freons went into production: $\mathrm{HFC}-134 \mathrm{a}\left(\mathrm{CH}_{2} \mathrm{FCF}_{3}\right)$ and \(\mathrm{HCFC}-124\left(\mathrm{CHCIFCF}_{3}\right)\) Calculate the molar masses of these two compounds.

Short Answer

Expert verified
The molar masses of the two compounds are: HFC-134a (CH2FCF3): \(90.03\ g/mol\) and HCFC-124 (CHClFCF3): \(124.47\ g/mol\).

Step by step solution

01

Calculate molar mass of HFC-134a (CH2FCF3)

To calculate the molar mass of HFC-134a, we first need to determine the molar mass of each element in the formula: - Carbon (C): 12.01 g/mol - Hydrogen (H): 1.01 g/mol - Fluorine (F): 19.00 g/mol Now, we can determine the molar mass of the compound: Molar mass of HFC-134a = (1 x 12.01) + (2 x 1.01) + (1 x 19.00) + (3 x 19.00) Molar mass of HFC-134a = 12.01 + 2.02 + 19.00 + 57.00 Molar mass of HFC-134a = 90.03 g/mol
02

Calculate molar mass of HCFC-124 (CHClFCF3)

To calculate the molar mass of HCFC-124, we first need to determine the molar mass of each element in the formula: - Carbon (C): 12.01 g/mol - Hydrogen (H): 1.01 g/mol - Chlorine (Cl): 35.45 g/mol - Fluorine (F): 19.00 g/mol Now, we can determine the molar mass of the compound: Molar mass of HCFC-124 = (1 x 12.01) + (1 x 1.01) + (1 x 35.45) + (1 x 19.00) + (3 x 19.00) Molar mass of HCFC-124 = 12.01 + 1.01 + 35.45 + 19.00 + 57.00 Molar mass of HCFC-124 = 124.47 g/mol So, the molar masses of the two compounds are: - HFC-134a (CH2FCF3): 90.03 g/mol - HCFC-124 (CHClFCF3): 124.47 g/mol

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Most popular questions from this chapter

Vitamin A has a molar mass of 286.4 \(\mathrm{g} / \mathrm{mol}\) and a general molecular formula of \(\mathrm{C}_{x} \mathrm{H}, \mathrm{E}\) , where \(\mathrm{E}\) is an unknown element. If vitamin \(\mathrm{A}\) is 83.86$\% \mathrm{C}\( and 10.56\)\% \mathrm{H}$ by mass, what is the molecular formula of vitamin A?

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