You have a gas sample of carbon dioxide at 298 K in a 2.00 L container containing 0.500 mol of CO_2. Using the ideal gas law, what is the pressure of your gas sample in atm?

• A. 12.2 atm
• B. 6.12 atm
• C. 0.082 atm
• D. 2.03 atm

Answer: (B)

Verified step by step guidance

1. Identify the known variables from the problem: number of moles \(n = 0.500\) mol, temperature \(T = 298\) K, volume \(V = 2.00\) L, and the ideal gas constant \(R = 0.0821\) L·atm/(mol·K).
2. Recall the ideal gas law equation: \(P \times V = n \times R \times T\), 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: \(P = \frac{0.500 \times 0.0821 \times 298}{2.00}\).
5. Calculate the value from the substitution to find the pressure \(P\) in atm.