9. What is the volume of \( 8.7 \times 10^{23} \) molecules of chlorine gas \( \left(\mathrm{Cl}_{2}\right) \) ?

To find the volume of \( 8.7 \times 10^{23} \) molecules of chlorine gas \( (\mathrm{Cl}_{2}) \), we first use Avogadro's number, which is approximately \( 6.022 \times 10^{23} \) molecules per mole. 1. Calculate the number of moles: \[ \text{Moles of } Cl_2 = \frac{8.7 \times 10^{23}}{6.022 \times 10^{23}} \approx 1.44 \text{ moles} \] 2. Knowing that one mole of any ideal gas occupies 22.4 liters at standard temperature and pressure (STP), we calculate the volume: \[ \text{Volume} = 1.44 \text{ moles} \times 22.4 \text{ L/mole} \approx 32.3 \text{ liters} \] So, the volume of \( 8.7 \times 10^{23} \) molecules of chlorine gas is approximately **32.3 liters**.