Determine the volume, in liters, occupied by 0.030 moles of a gas at STP.

To determine the volume of a gas at standard temperature and pressure (STP), we can use the ideal gas law or the known molar volume at STP.

At STP:
- **Temperature** = 273.15 K
- **Pressure** = 1 atm
- **Molar volume of an ideal gas at STP** = 22.4 liters per mole

Given that you have 0.030 moles of the gas, the volume \( V \) occupied by the gas can be calculated using the proportional relationship:

\[
V = n \times 22.4 \text{ L/mol}
\]

Where:
- \( n \) is the number of moles.

Now, substituting the values:

\[
V = 0.030 \text{ mol} \times 22.4 \text{ L/mol}
\]
\[
V = 0.672 \text{ L}
\]

So, the gas occupies **0.672 liters** at STP.

Would you like a detailed explanation of the STP conditions or ideal gas law?

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Here are 5 related questions to expand your understanding:
1. How is the molar volume of an ideal gas derived at STP?
2. How does the volume of gas change with temperature at constant pressure?
3. What is the ideal gas law and how can it be applied to real gases?
4. What happens to the volume of a gas if the pressure is doubled at constant temperature?
5. How would the volume change if the amount of gas were doubled?

**Tip:** Always ensure that temperature and pressure are in consistent units when using the ideal gas law!

Discover how to calculate the volume occupied by 0.030 moles of a gas at STP using the molar volume of 22.4 L/mol. This problem explores key concepts from stoichiometry and gas laws, suitable for high school students in Grades 10-12.

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