Question

1. how much would a sample of 28.3 x 10²⁴ atoms of carbon weigh in grams?

Explanation:

Step1: Calculate the number of moles

Use Avogadro's number ($N_A = 6.022\times10^{23}$ atoms/mol). The number of moles ($n$) of carbon is given by $n=\frac{N}{N_A}$, where $N = 28.3\times10^{24}$ atoms.
$$n=\frac{28.3\times 10^{24}}{6.022\times 10^{23}}=\frac{28.3}{6.022}\times10\approx46.99\ mol$$

Step2: Calculate the mass

The molar mass of carbon ($M$) is $12.01\ g/mol$. The mass ($m$) is calculated using the formula $m = n\times M$.
$$m=46.99\times12.01\approx564.35\ g$$

Answer:

$564.35\ g$