What is the mass of 4.91×10²¹ platinum atoms?

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Determine the molar mass of platinum (Pt) from the periodic table, which is approximately 195.08 g/mol.

Use Avogadro's number, which is approximately 6.022 \(\times\) 10^{23} atoms/mol, to find the number of moles of platinum atoms in 4.91 \(\times\) 10^{21} atoms.

Calculate the number of moles of platinum by dividing the given number of atoms by Avogadro's number: \(\text{moles of Pt}\) = \(\frac{4.91 \times 10^{21}\) \(\text{ atoms}\)}{6.022 \(\times\) 10^{23} \(\text{ atoms/mol}\)}.

Multiply the number of moles of platinum by the molar mass of platinum to find the mass: \(\text{mass of Pt}\) = \(\text{moles of Pt}\) \(\times\) 195.08 \(\text{ g/mol}\).

The result from the previous step will give you the mass of 4.91 \(\times\) 10^{21} platinum atoms in grams.

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주요 개념

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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For platinum, the molar mass is approximately 195.08 g/mol. This value is essential for converting between the number of atoms and the mass of the substance, as it allows us to relate the atomic scale to macroscopic quantities.

Avogadro's Number

Avogadro's number, approximately 6.022 x 10²³, is the number of atoms, ions, or molecules in one mole of a substance. This constant is crucial for converting between the number of individual atoms and moles, enabling calculations involving quantities of matter in chemical reactions and stoichiometry.

Conversion of Atoms to Mass

To find the mass of a specific number of atoms, one must first convert the number of atoms to moles using Avogadro's number, and then multiply the number of moles by the molar mass of the element. This process allows for the determination of the mass of a given quantity of atoms, which is fundamental in stoichiometric calculations in chemistry.

What is the mass of 4.91×1021 platinum atoms?