A 2.49 g sample of a gas occupies 752 mL at 1.98 atm and 62 °C. Based on these data, the gas is most likely:

• A. SO2
• B. N2
• C. O2
• D. CO2

Answer: (C)

Verified step by step guidance

1. Identify the known variables from the problem: mass (m) = 2.49 g, volume (V) = 752 mL (convert to liters by dividing by 1000), pressure (P) = 1.98 atm, and temperature (T) = 62 °C (convert to Kelvin by adding 273.15).
2. Use the Ideal Gas Law equation to find the number of moles (n) of the gas: \(P \times V = n \times R \times T\), where \(R\) is the ideal gas constant (0.0821 L\cdot atm / mol\cdot K). Rearrange to solve for \(n\): \(n = \frac{P \times V}{R \times T}\).
3. Calculate the molar mass (M) of the gas using the formula \(M = \frac{\text{mass}}{n}\), where mass is in grams and \(n\) is the number of moles calculated in the previous step.
4. Compare the calculated molar mass to the molar masses of the given gases: SO\(_2\) (64.07 g/mol), N\(_2\) (28.02 g/mol), O\(_2\) (32.00 g/mol), and CO\(_2\) (44.01 g/mol).
5. Determine which gas has a molar mass closest to the calculated value to identify the most likely gas sample.