Using the ideal gas law, what pressure (in atm) will be exerted by 1.5 moles of neon gas occupying 5.0 L at 273 K?

• A. 6.7 atm
• B. 1.8 atm
• C. 0.67 atm
• D. 13.4 atm

Answer: (A)

Verified step by step guidance

1. Identify the known variables from the problem: number of moles \(n = 1.5\) mol, volume \(V = 5.0\) L, and temperature \(T = 273\) K.
2. Recall the ideal gas law formula: \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
3. Choose the appropriate value for the ideal gas constant \(R\) that matches the units of pressure in atm, volume in liters, and temperature in Kelvin. This value is \(R = 0.0821 \frac{L \cdot atm}{mol \cdot K}\).
4. Rearrange the ideal gas law to solve for pressure \(P\): \(P = \frac{n \times R \times T}{V}\)
5. Substitute the known values into the equation: \(P = \frac{1.5 \times 0.0821 \times 273}{5.0}\) Then calculate the pressure to find the answer.