What is the mass in grams of 5.67 x 1022 molecules of O2 (32.00 g/mol)?

To find the mass in grams of 5.67 x 10²² molecules of O₂, we will use the following steps:

1. **Find the molar mass of O₂**:  
   The molar mass of oxygen (O₂) is given as 32.00 g/mol. 

2. **Use Avogadro's number**:  
   Avogadro's number tells us that 1 mole of any substance contains \( 6.022 \times 10^{23} \) molecules. We will use this to determine how many moles correspond to 5.67 x 10²² molecules.

3. **Set up a ratio**:  
   The number of moles (n) can be found by dividing the number of molecules by Avogadro's number:
   \[
   n = \frac{\text{Number of molecules}}{6.022 \times 10^{23}}
   \]
   \[
   n = \frac{5.67 \times 10^{22}}{6.022 \times 10^{23}} = 0.0942 \text{ moles}
   \]

4. **Calculate the mass**:  
   Finally, multiply the number of moles by the molar mass of O₂ to get the mass in grams:
   \[
   \text{Mass} = n \times \text{Molar mass}
   \]
   \[
   \text{Mass} = 0.0942 \times 32.00 = 3.0144 \text{ grams}
   \]

So, the mass of 5.67 x 10²² molecules of O₂ is approximately **3.01 grams**.

Would you like any further details or clarifications?

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Here are 5 related questions:
1. How do you calculate the number of moles from a given number of atoms or molecules?
2. What is Avogadro's number and why is it useful in chemistry?
3. How would the calculation change if you had a different molar mass, say for H₂O?
4. What are the differences between atomic mass and molar mass?
5. How can we experimentally determine the molar mass of a compound?

**Tip**: When dealing with molecules and atoms, always keep track of whether you’re calculating for individual atoms or molecules, since it affects the molar mass and other quantities.

What is the mass in grams of 5.67 x 10²² molecules of O₂ (32.00 g/mol)?

Learn how to calculate the mass of 5.67 x 10²² molecules of O₂ using molar mass (32.00 g/mol) and Avogadro's number. This chemistry problem involves key concepts like molar mass and ratio setup, suitable for students in Grades 10-12.

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