A chemist wishes to prepare `6.022 xx 10^24` molecules of `SO_(2)` according to the reaction :
`S+O_(2) to SO_(2)`
How many gram atoms of S and how many grams of O does he need ?

Explanation

To solve the problem of how many gram atoms of sulfur (S) and how many grams of oxygen (O) are needed to prepare \(6.022 \times 10^{24}\) molecules of \(SO_2\), we will follow these steps:

### Step 1: Determine the number of moles of \(SO_2\)
Using Avogadro's number, which states that \(1\) mole of any substance contains \(6.022 \times 10^{23}\) molecules, we can calculate the number of moles of \(SO_2\) needed.

\[ \text{Number of moles of } SO_2 = \frac{6.022 \times 10^{24} \text{ molecules}}{6.022 \times 10^{23} \text{ molecules/mole}} = 10 \text{ moles} \]
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