Question
how many atoms of neon gas would a container with a volume of 67.2L hold at STP
Answers
GPT-4o mini
To calculate the number of atoms of neon gas in a container with a volume of 67.2 liters at Standard Temperature and Pressure (STP), we will use the molar volume of an ideal gas at STP, which is approximately 22.4 liters per mole.
1. **Calculate the number of moles of neon gas:**
\[
\text{Number of moles} = \frac{\text{Volume of gas}}{\text{Molar volume at STP}} = \frac{67.2 \, \text{L}}{22.4 \, \text{L/mol}} \approx 3.00 \, \text{moles}
\]
2. **Calculate the number of atoms in the moles of neon:**
Since one mole of any substance contains Avogadro's number of entities (atoms, molecules, etc.), which is approximately \(6.022 \times 10^{23}\):
\[
\text{Number of atoms} = \text{Number of moles} \times \text{Avogadro's number} = 3.00 \, \text{moles} \times 6.022 \times 10^{23} \, \text{atoms/mole}
\]
\[
\text{Number of atoms} \approx 1.81 \times 10^{24} \, \text{atoms}
\]
Therefore, a container with a volume of 67.2 L of neon gas at STP would hold approximately \(1.81 \times 10^{24}\) atoms of neon.
1. **Calculate the number of moles of neon gas:**
\[
\text{Number of moles} = \frac{\text{Volume of gas}}{\text{Molar volume at STP}} = \frac{67.2 \, \text{L}}{22.4 \, \text{L/mol}} \approx 3.00 \, \text{moles}
\]
2. **Calculate the number of atoms in the moles of neon:**
Since one mole of any substance contains Avogadro's number of entities (atoms, molecules, etc.), which is approximately \(6.022 \times 10^{23}\):
\[
\text{Number of atoms} = \text{Number of moles} \times \text{Avogadro's number} = 3.00 \, \text{moles} \times 6.022 \times 10^{23} \, \text{atoms/mole}
\]
\[
\text{Number of atoms} \approx 1.81 \times 10^{24} \, \text{atoms}
\]
Therefore, a container with a volume of 67.2 L of neon gas at STP would hold approximately \(1.81 \times 10^{24}\) atoms of neon.