A 5.00 L tank contains 2.50 moles of oxygen gas at 39.3 °C. What is the pressure in atm inside the tank? (R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 10.1 atm
• B. 8.2 atm
• C. 14.0 atm
• D. 13.2 atm

Answer: (C)

Verified step by step guidance

1. Identify the known variables from the problem: number of moles \(n = 2.50\) mol, volume \(V = 5.00\) L, temperature \(T = 39.3\ ^\circ\mathrm{C}\), and the gas constant \(R = 0.0821\ \mathrm{L \cdot atm \cdot mol^{-1} \cdot K^{-1}}\).
2. Convert the temperature from Celsius to Kelvin using the formula: \(T(K) = T(^\circ C) + 273.15\). So, calculate \(T = 39.3 + 273.15\) K.
3. Use the Ideal Gas Law equation to relate pressure, volume, moles, and temperature: \(P V = n R T\).
4. Rearrange the Ideal Gas Law to solve for pressure \(P\): \(P = \frac{n R T}{V}\).
5. Substitute the known values of \(n\), \(R\), \(T\) (in Kelvin), and \(V\) into the equation and calculate the pressure \(P\) in atm.