A 5.00 L tank contains 10.00 grams of oxygen gas (O_2) at a temperature of 350 K. What is the pressure in the tank in atmospheres (atm)? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 0.56 atm
• B. 0.88 atm
• C. 2.24 atm
• D. 1.40 atm

Answer: (D)

Verified step by step guidance

1. Identify the known quantities: volume \(V = 5.00\ \text{L}\), mass of oxygen \(m = 10.00\ \text{g}\), temperature \(T = 350\ \text{K}\), and the gas constant \(R = 0.0821\ \text{L} \cdot \text{atm} \cdot \text{mol}^{-1} \cdot \text{K}^{-1}\).
2. Calculate the number of moles of oxygen gas using its molar mass. The molar mass of \(O_2\) is approximately \$32.00\ \text{g/mol}\(. Use the formula: \)n = \frac{m}{M}\(, where \)n\( is moles, \)m\( is mass, and \)M$ is molar mass.
3. Apply the ideal gas law equation to find the pressure: \(P V = n R T\). Rearrange to solve for pressure \(P\): \(P = \frac{n R T}{V}\).
4. Substitute the values of \(n\), \(R\), \(T\), and \(V\) into the equation to express pressure in terms of the known quantities.
5. Perform the calculation to find the pressure in atmospheres, ensuring units are consistent throughout the process.