A rigid container holds a gas at a pressure of 11 atm, a volume of 2.0 L, and a temperature of 300 K. Using the ideal gas law, how many moles of gas are present in the container?

• A. 1.10 mol
• B. 0.61 mol
• C. 0.73 mol
• D. 0.90 mol

Answer: (D)

Verified step by step guidance

1. Identify the known variables from the problem: pressure \(P = 11\) atm, volume \(V = 2.0\) L, and temperature \(T = 300\) K.
2. Recall the ideal gas law equation: \(P \times V = n \times R \times T\), where \(n\) is the number of moles and \(R\) is the ideal gas constant.
3. Choose the appropriate value for the ideal gas constant \(R\) that matches the units of pressure in atm and volume in liters, which is \(R = 0.0821 \ \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K}\).
4. Rearrange the ideal gas law to solve for the number of moles \(n\): \(n = \frac{P \times V}{R \times T}\)
5. Substitute the known values into the rearranged equation to find \(n\): \(n = \frac{11 \ \text{atm} \times 2.0 \ \text{L}}{0.0821 \ \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K} \times 300 \ \text{K}}\)