객관식
How many molecules of O_2 occupy a volume of 1.0 L at 65 °C and 778 mm Hg? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1} and 1 atm = 760 mm Hg.)
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7. Gases
The Ideal Gas Law
객관식
According to the ideal gas law, what volume would be occupied by 2.00 moles of propane gas (C_3H_8) at standard temperature and pressure (STP)?
A
2.00 L
B
44.8 L
C
22.4 L
D
11.2 L
검증된 단계별 안내1
Identify the known variables: number of moles \(n = 2.00\) moles, temperature \(T = 273.15\ \text{K}\) (standard temperature), and pressure \(P = 1.00\ \text{atm}\) (standard pressure).
Recall the ideal gas law equation: \(P \times V = n \times R \times T\), where \(V\) is the volume, \(R\) is the ideal gas constant, \(P\) is pressure, \(n\) is moles, and \(T\) is temperature.
Use the ideal gas constant \(R = 0.0821\ \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K}\), which is appropriate for these units.
Rearrange the ideal gas law to solve for volume \(V\):
\(V = \frac{n \times R \times T}{P}\)
Substitute the known values into the equation:
\(V = \frac{2.00 \times 0.0821 \times 273.15}{1.00}\), then calculate to find the volume occupied by the propane gas at STP.
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