A sample of gas is contained in a 5.0 L vessel at a temperature of 373 K and a pressure of 203 kPa. Using the ideal gas law, how many moles of gas are present in the container? (Use R = 8.314 L·kPa·K^{-1}·mol^{-1})

• A. 0.60 mol
• B. 0.25 mol
• C. 0.45 mol
• D. 0.33 mol

Answer: (D)

Verified step by step guidance

1. Identify the known variables from the problem: volume \(V = 5.0\ \text{L}\), temperature \(T = 373\ \text{K}\), pressure \(P = 203\ \text{kPa}\), and the ideal gas constant \(R = 8.314\ \text{L} \cdot \text{kPa} \cdot \text{K}^{-1} \cdot \text{mol}^{-1}\).
2. Recall the ideal gas law formula: \(P \times V = n \times R \times T\), where \(n\) is the number of moles of gas.
3. Rearrange the ideal gas law to solve for \(n\): \(n = \frac{P \times V}{R \times T}\).
4. Substitute the known values into the rearranged formula: \(n = \frac{203 \times 5.0}{8.314 \times 373}\).
5. Perform the arithmetic to calculate \(n\), which will give the number of moles of gas present in the container.