A 9.00 L tank contains 75.1 grams of fluorine gas (F_2) at a temperature of 355 K. What is the pressure inside the tank? (R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 3.18 atm
• B. 6.37 atm
• C. 1.59 atm
• D. 12.7 atm

Answer: (B)

Verified step by step guidance

1. First, calculate the number of moles of fluorine gas (F_2) using its molar mass. The molar mass of F_2 is approximately 38.00 g/mol. Use the formula: \(n = \frac{\text{mass}}{\text{molar mass}} = \frac{75.1\ \text{g}}{38.00\ \text{g/mol}}\).
2. Next, use the Ideal Gas Law equation to relate pressure, volume, moles, and temperature: \(P V = n R T\), where \(P\) is pressure, \(V\) is volume, \(n\) is moles, \(R\) is the gas constant, and \(T\) is temperature in Kelvin.
3. Rearrange the Ideal Gas Law to solve for pressure: \(P = \frac{n R T}{V}\).
4. Substitute the known values into the equation: \(n\) from step 1, \(R = 0.0821\ \text{L·atm·mol}^{-1}\text{·K}^{-1}\), \(T = 355\ \text{K}\), and \(V = 9.00\ \text{L}\).
5. Calculate the pressure \(P\) using the substituted values to find the pressure inside the tank.