In an ideal gas law experiment, a student collects 0.50 mol of a gas in a 10.0 L container at 300 K. What is the pressure of the gas in atmospheres? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 0.82 atm
• B. 0.50 atm
• C. 2.05 atm
• D. 1.23 atm

Answer: (D)

Verified step by step guidance

1. Identify the known variables from the problem: number of moles \(n = 0.50\) mol, volume \(V = 10.0\) L, temperature \(T = 300\) K, and the gas constant \(R = 0.0821\) L\cdot atm\cdot mol^{-1}\cdot K^{-1}$.
2. Recall the Ideal Gas Law equation: \(P V = n R T\), where \(P\) is the pressure in atmospheres.
3. Rearrange the Ideal Gas Law to solve for pressure \(P\): \(P = \frac{n R T}{V}\).
4. Substitute the known values into the equation: \(P = \frac{0.50 \times 0.0821 \times 300}{10.0}\).
5. Calculate the value from the substitution to find the pressure \(P\) in atmospheres.