A 6.00 L tank contains 20.0 grams of nitrogen gas (N_2) at a temperature of 385 K. What is the pressure inside the tank? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 2.60 atm
• B. 0.98 atm
• C. 4.10 atm
• D. 1.85 atm

Answer: (A)

Verified step by step guidance

1. Identify the known quantities: volume (V) = 6.00 L, mass of nitrogen gas (m) = 20.0 g, temperature (T) = 385 K, and the gas constant (R) = 0.0821 L\cdot atm\cdot mol^{-1}\cdot K^{-1}.
2. Calculate the number of moles (n) of nitrogen gas using its molar mass. The molar mass of N_2 is approximately 28.0 g/mol. Use the formula: \(n = \frac{m}{\text{molar mass}}\).
3. Apply the ideal gas law equation to find the pressure: \(P V = n R T\). Rearrange to solve for pressure: \(P = \frac{n R T}{V}\).
4. Substitute the values of n, R, T, and V into the equation to express the pressure in atm.
5. Perform the calculation to find the pressure inside the tank.