Question

current attempt in progress
the actual mass of an atom of cl is 5.886×10⁻²³ g. how many atoms of cl are in a 10.0 g sample?
5.89×10⁻²⁴ atoms
1.70×10²³ atoms
5.87×10²³ atoms
1.70×10⁻²³ atoms
35.0 atoms

Explanation:

Step1: Identify the formula

To find the number of atoms, use the formula $n=\frac{m_{total}}{m_{atom}}$, where $n$ is the number of atoms, $m_{total}$ is the total mass of the sample and $m_{atom}$ is the mass of one - atom.

Step2: Substitute the given values

We have $m_{total} = 10.0\ g$ and $m_{atom}=5.886\times 10^{-23}\ g$. So $n=\frac{10.0}{5.886\times 10^{-23}}$.

Step3: Calculate the result

$n=\frac{10.0}{5.886\times 10^{-23}}=\frac{10.0}{5.886}\times10^{23}\approx1.70\times 10^{23}$ atoms.

Answer:

B. $1.70\times 10^{23}$ atoms