Answer: " [tex]1.41 * 10^{24}[/tex] " atoms of aluminum (Al) .
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Explanation:
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Using a technique called "dimensional analysis" ; as follows:
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→ " [tex]\frac{2.34 mol Al}{1} * \frac{6.022*10^{23}atoms Al}{1 mol Al} = ?[/tex]
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The units "mol Al" ["moles of aluminum"] cancel out; and we have:
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→ "[tex][(2.34) * (6.022 * 10^{23})] = ?[/tex] atoms of Al [aluminum].
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Note that by definition: 1 (one) "mole" (abbreviated "mol") of anything consists of " [tex]6.022*10^{23}[/tex] " units " of that particular thing.
This number: 6.022*10^{23} —is known as: "Avogadro's number".
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→ [ 2.34 * 6.022 * 10^23] ;
= 1.409148 * 10^24 ;
→ Round to 3 (Three) significant figures;
→ since: "2.34" has 3 (Three) significant figures;
→ to get: " [tex]1.41 *10^{24}[/tex] atoms of aluminum (Al).
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Hope this is helpful to you! Wishing you the best!
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