QuestionAugust 12, 2025

The formula for sulfur hexafluoride is SF_(6) a. How many molecules are in 2.60 grams of sulfur hexafluoride? square molecules b. What is the mass in grams of 2.17times 10^22 molecules of sulfur hexafluoride? square grams

The formula for sulfur hexafluoride is SF_(6) a. How many molecules are in 2.60 grams of sulfur hexafluoride? square molecules b. What is the mass in grams of 2.17times 10^22 molecules of sulfur hexafluoride? square grams
The formula for sulfur hexafluoride is SF_(6) a. How many molecules are in 2.60 grams of sulfur hexafluoride? square molecules b. What is the mass in grams of 2.17times 10^22 molecules of sulfur hexafluoride? square grams

Solution
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Answer

a. 1.07 \times 10^{22} molecules ### b. 5.26 grams Explanation 1. Calculate Molar Mass of SF_6 Sulfur (S) has a molar mass of 32.07 g/mol, and Fluorine (F) has a molar mass of 19.00 g/mol. For SF_6, the molar mass is 32.07 + 6 \times 19.00 = 146.07 g/mol. 2. Convert Grams to Moles for Part (a) Use the formula: **moles = \frac{\text{mass}}{\text{molar mass}}**. For 2.60 grams, moles = \frac{2.60}{146.07}. 3. Convert Moles to Molecules for Part (a) Use Avogadro's number: **molecules = \text{moles} \times 6.022 \times 10^{23}**. Calculate molecules using the moles from Step 2. 4. Convert Molecules to Moles for Part (b) Use the formula: **moles = \frac{\text{molecules}}{6.022 \times 10^{23}}**. For 2.17\times 10^{22} molecules, calculate moles. 5. Convert Moles to Grams for Part (b) Use the formula: **mass = \text{moles} \times \text{molar mass}**. Calculate mass using the moles from Step 4.

Explanation

1. Calculate Molar Mass of $SF_6$<br /> Sulfur (S) has a molar mass of 32.07 g/mol, and Fluorine (F) has a molar mass of 19.00 g/mol. For $SF_6$, the molar mass is $32.07 + 6 \times 19.00 = 146.07$ g/mol.<br /><br />2. Convert Grams to Moles for Part (a)<br /> Use the formula: **moles = \frac{\text{mass}}{\text{molar mass}}**. For 2.60 grams, moles = $\frac{2.60}{146.07}$.<br /><br />3. Convert Moles to Molecules for Part (a)<br /> Use Avogadro's number: **molecules = \text{moles} \times 6.022 \times 10^{23}**. Calculate molecules using the moles from Step 2.<br /><br />4. Convert Molecules to Moles for Part (b)<br /> Use the formula: **moles = \frac{\text{molecules}}{6.022 \times 10^{23}}**. For $2.17\times 10^{22}$ molecules, calculate moles.<br /><br />5. Convert Moles to Grams for Part (b)<br /> Use the formula: **mass = \text{moles} \times \text{molar mass}**. Calculate mass using the moles from Step 4.
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