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QuestionAnatomy and Physiology

The molar mass of silver $(\mathrm{Ag})$ is $107.87 \mathrm{~g} / \mathrm{mol}$. Calculate the mass in grams of a sample of Ag containing $1.97 \times 10^{22}$ atoms. Write your answer using three significant figures. $\square$

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Step 1
: Write down the relationship between the number of atoms, the molar mass, and the mass of a substance.

where $m$ is the mass of the sample, $N$ is the number of atoms in the sample, $M$ is the molar mass of the substance, and $N_A$ is Avogadro's number, which is approximately $6.022 \times 10^{23} \text{ atoms/mol}$.
The number of atoms in a sample is related to the mass of the sample through the molar mass of the substance. This relationship is given by the following equation:

Step 2
: Plug in the given values into the equation.

m=(1.97×1022) atoms×107.87 g/mol6.022×1023 atoms/molm = (1.97 \times 10^{22}) \text{ atoms} \times \frac{107.87 \text{ g/mol}}{6.022 \times 10^{23} \text{ atoms/mol}}
Plug these values into the equation:

Final Answer

is $35.4 \text{ g}$.

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