Using the ideal gas law, what is the pressure (in atm) of 1.9 mol of nitrogen gas in a 9.45 L tank at a temperature of 228 K? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 0.40 atm
• B. 0.40 atm
• C. 0.38 atm
• D. 0.48 atm

Answer: (C)

Verified step by step guidance

1. Identify the known variables from the problem: number of moles \(n = 1.9\) mol, volume \(V = 9.45\) L, temperature \(T = 228\) K, and the ideal gas constant \(R = 0.0821\) L\cdot atm\cdot mol^{-1}\cdot K^{-1}$.
2. Recall the ideal gas law formula: \(P \times V = n \times R \times T\), where \(P\) is the pressure in atm.
3. Rearrange the ideal gas law to solve for pressure \(P\): \(P = \frac{n \times R \times T}{V}\).
4. Substitute the known values into the equation: \(P = \frac{1.9 \times 0.0821 \times 228}{9.45}\).
5. Perform the multiplication and division to calculate the pressure \(P\) in atm.