Put it all together to complete this problem:
10. A student measured out 75.8 g of carbon dioxide, , in the laboratory. How
many moles of carbon dioxide did the student measure?

To determine the number of moles of carbon dioxide, you can use the formula: moles = mass (g) / molar mass (g/mol). The molar mass of is approximately 44.01 g/mol (12.01 g/mol for carbon and 16.00 g/mol for each oxygen). Using the mass measured, the calculation would be:

Moles of = 75.8 g / 44.01 g/mol ≈ 1.72 moles.

And there you have it! The student measured approximately 1.72 moles of carbon dioxide.

Did you know that carbon dioxide is naturally present in Earth’s atmosphere and plays a crucial role in the carbon cycle? It’s produced by various processes including respiration, combustion, and decay of organic matter. This simple yet vital molecule helps sustain life on our planet!

For real-world applications, carbon dioxide is not just a byproduct of life; it’s also used in carbonation of beverages, fire extinguishers, and even agricultural practices to enhance plant growth in greenhouses. Understanding its properties and behaviors is key to harnessing its potential across various industries!