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Chapter 9: Problem 67

Consider a sample of \(24.0 \mathrm{~g}\) of \(\mathrm{O}_{2}\) molecules. (a) How many moles of \(\mathrm{O}_{2}\) molecules are present? (b) How many moles of \(\mathrm{O}\) atoms are present?

Short Answer

Expert verified
(a) There are \(0.75 \mathrm{mol}\) of O₂ molecules in the sample. (b) There are \(1.5 \mathrm{mol}\) of O atoms in the sample.

Step by step solution

01

Calculate the moles of O₂ molecules

To find out the moles of O₂ molecules, we need to use the formula: \[ moles = \frac{mass}{molar\,mass} \] The given mass of the O₂ molecules is \(24.0 \mathrm{g}\), and the molar mass of O₂ is the sum of two oxygen atoms, and as each oxygen atom has a mass of \(16.0 \mathrm{g/mol}\), the molar mass of O₂ is \(32.0 \mathrm{g/mol}\). Now we can calculate the number of moles: \[ moles\,of\,O₂ = \frac{24.0 \mathrm{g}}{32.0 \mathrm{g/mol}} = 0.75 \mathrm{mol} \]
02

Calculate the moles of O atoms

Knowing the moles of O₂ molecules, we can determine the number of moles of O atoms in the sample. Since each O₂ molecule contains two O atoms, the number of moles of O atoms will be double the number of O₂ moles: \[ moles\,of\,O = 2 \times moles\,of\,O₂ \] \[ moles\,of\,O = 2 \times 0.75 \mathrm{mol} = 1.5 \mathrm{mol} \] The answer to the questions is: (a) There are \(0.75 \mathrm{mol}\) of O₂ molecules in the sample. (b) There are \(1.5 \mathrm{mol}\) of O atoms in the sample.

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Most popular questions from this chapter

Consider the unbalanced chemical equation \(\mathrm{CaC}_{2}+\mathrm{CO} \rightarrow \mathrm{C}+\mathrm{CaCO}_{3}\) When the reaction is complete, \(135.4 \mathrm{~g}\) of \(\mathrm{CaCO}_{3}\) produced and \(38.5 \mathrm{~g}\) of \(\mathrm{CaC}_{2}\) is left over. Assuming the reaction had a \(100 \%\) yield, what were the mass of the two reactants at the beginning of the reaction

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