Multiple Choice
A condensation reaction involving 200 glucose molecules, C6H12O6, results in a polysaccharide. What is the molar mass, in g/mol, of the polysaccharide, assuming complete reaction and loss of water molecules?
2. Atoms & Elements
Calculating Molar Mass
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How many fluorine atoms are present in 135 g of CF2Cl2?
A
1.58 x 10^24 fluorine atoms
B
7.90 x 10^23 fluorine atoms
C
3.16 x 10^24 fluorine atoms
D
6.02 x 10^23 fluorine atoms
Verified step by step guidance1
First, determine the molar mass of CF2Cl2. Calculate the molar mass by adding the atomic masses of each element in the compound: Carbon (C), Fluorine (F), and Chlorine (Cl). Use the periodic table to find these values: C = 12.01 g/mol, F = 19.00 g/mol, Cl = 35.45 g/mol.
Calculate the molar mass of CF2Cl2 using the formula: \( \text{Molar mass of CF}_2\text{Cl}_2 = 12.01 + (2 \times 19.00) + (2 \times 35.45) \).
Convert the given mass of CF2Cl2 (135 g) to moles using the molar mass calculated in the previous step. Use the formula: \( \text{moles of CF}_2\text{Cl}_2 = \frac{\text{mass of CF}_2\text{Cl}_2}{\text{molar mass of CF}_2\text{Cl}_2} \).
Determine the number of fluorine atoms in the moles of CF2Cl2 calculated. Since each molecule of CF2Cl2 contains 2 fluorine atoms, multiply the moles of CF2Cl2 by Avogadro's number (\(6.022 \times 10^{23}\) molecules/mol) and then by 2 to find the total number of fluorine atoms.
Finally, express the number of fluorine atoms in scientific notation to match the format of the given answer choices.
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