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Answer :
Final answer:
Approximately 0.0560 grams of aluminum is equivalent to 1.25 x 10^21 atoms. None of the provided options (A) 13.1 grams, (B) 26.98 grams, (C) 39.1 grams, (D) 52.88 grams) are correct.
Explanation:
To answer this question, we need to understand a few terms in chemistry - the atomic mass unit (AMU) and Avogadro's number. The atomic mass of aluminum is approximately 26.98 AMU. In chemistry, AMU acts as a bridge between the atomic and macro worlds, since 1 mole of any substance contains Avogadro's number (approximately 6.022 x 10^23) of entities (atoms in this case).
This implies that 1 mole of aluminum (approximately 26.98 grams) contains 6.022 x 10^23 atoms. Hence, if we know the number of atoms, we can identify the equivalent weight in grams.
The number of moles of aluminum in 1.25 x 10^21 atoms can be calculated as: (1.25 x 10^21 atoms) / (6.022 x 10^23 atoms/mole) = 2.076 x10^-3 moles.
The corresponding weight in grams is then: (2.076 x 10^-3 moles) x (26.98 grams/mole) = 0.0560 grams.
So, none of the options provided are correct as 1.25 x 10^21 atoms of aluminum weigh approximately 0.0560 grams, not 13.1 grams, 26.98 grams, 39.1 grams, or 52.88 grams.
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