Calculate the mass, in grams, of each sample. d. 7.9×10²¹ uranium atoms

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Determine the molar mass of uranium (U) from the periodic table. Uranium has an atomic mass of approximately 238 g/mol.

Calculate the number of moles of uranium atoms present in the sample using Avogadro's number (6.022 \(\times\) 10^{23} atoms/mol). Use the formula: \(\text{moles}\) = \(\frac{\text{number of atoms}\)}{\(\text{Avogadro's number}\)}.

Multiply the number of moles of uranium by the molar mass of uranium to find the mass of the sample in grams. Use the formula: \(\text{mass}\) = \(\text{moles}\) \(\times\) \(\text{molar mass}\).

Ensure all units are consistent (moles, grams) throughout the calculation to avoid any errors.

Double-check your calculations for any possible arithmetic errors to ensure the accuracy of your result.

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주요 개념

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Avogadro's Number

Avogadro's number, approximately 6.022 x 10^23, is the number of atoms, molecules, or particles in one mole of a substance. This constant allows chemists to convert between the number of particles and the amount of substance in moles, which is essential for stoichiometric calculations.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For uranium, the molar mass is approximately 238.03 g/mol. Knowing the molar mass is crucial for converting moles to grams, enabling the calculation of the mass of a given number of atoms.

Mass Calculation from Atoms

To calculate the mass of a sample from the number of atoms, one first converts the number of atoms to moles using Avogadro's number. Then, the number of moles is multiplied by the molar mass of the element to find the mass in grams. This process is fundamental in quantitative chemistry for determining the mass of elements in a sample.

Calculate the mass, in grams, of each sample. d. 7.9×1021 uranium atoms