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Consider the following reaction:

\[ \text{C}_7\text{H}_{16} + 11 \text{O}_2 \rightarrow 7 \text{CO}_2 + 8 \text{H}_2\text{O} \]

How many oxygen atoms are required to react with 35.9 g of \[\text{C}_7\text{H}_{16}\]?

Answer :

Final answer:

To react with 35.9g of C7H16, approximately 4.75x10^24 oxygen atoms are needed based on the balanced equation and molar calculations.

Explanation:

The subject of this question is about calculating the number of oxygen atoms required to react with a given amount of C7H16. From the balanced equation, we can see that 1 mole of C7H16 reacts with 11 moles of O2. The molecular weight of C7H16 is around 100.204 g/mol. Therefore, 35.9g of C7H16 is approximately 0.359 moles. Since we know that there are 11 moles of oxygen for each mole of C7H16 in the balanced chemical reaction, the number of moles of oxygen needed would be 0.359 * 11 = 3.949 moles. Since one mole of oxygen O2 consists of two oxygen atoms, this means we require 3.949 * 2 = 7.898 moles of oxygen atoms. Since Avogadro's number tells us there are 6.022x10^23 atoms in a mole, we multiply this number by our moles of oxygen atoms to get approximately 4.75x10^24 oxygen atoms.

Learn more about Molar Calculations here:

https://brainly.com/question/33057890

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Rewritten by : Jeany

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