Calculate the mass (in ng)of 2.33 × 10²⁰atoms of oxygen. A) 6.19 × 10⁶ ng B) 1.62 × 10⁷ ng C) 2.25 × 10³ ng D) 3.73 × 10⁶ ng E) 4.69 × 10⁷ ng

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Quizplus · Accepted Answer

To calculate the mass of $2.33 \times 10^{20}$ atoms of oxygen, first find the mass of one mole of oxygen atoms (16 g/mol for $O$, but since oxygen naturally exists as $O_2$, it's 32 g/mol for molecular oxygen, which is not relevant here as we're considering atomic oxygen). Then, use Avogadro's number ($6.022 \times 10^{23}$ atoms/mol) to find the mass of $2.33 \times 10^{20}$ atoms. The calculation is as follows: $\frac{16 g/mol}{6.022 \times 10^{23} atoms/mol} \times 2.33 \times 10^{20} atoms = 6.19 \times 10^{-3} g = 6.19 \times 10^{16} ng$.

Calculate the Mass (In Ng)of 2