Final answer:
The density of a gas at a given temperature and pressure can be determined using the ideal gas law equation. By rearranging the equation, we can calculate the densities of the given gases and determine that the gas with a density of 2.32 g/L is C4H10.
Step-by-step explanation:
The density of a gas at a given temperature and pressure can be determined using the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
To find the density of a gas, the ideal gas law equation can be rearranged to solve for density (d), which is equal to the mass (m) divided by the volume (V), d = m/V. Therefore, d = (P * M) / (R * T), where M is the molar mass of the gas.
Using this equation, we can calculate the densities of the given gases at the given temperature and pressure:
1) CO₂: d = (750 mmHg * 44.01 g/mol) / (0.0821 L*atm/mol*K * (27 + 273) K) = 1.79 g/L
2) Kr: d = (750 mmHg * 83.80 g/mol) / (0.0821 L*atm/mol*K * (27 + 273) K) = 4.88 g/L
3) H₂S: d = (750 mmHg * 34.08 g/mol) / (0.0821 L*atm/mol*K * (27 + 273) K) = 1.32 g/L
4) C4H10: d = (750 mmHg * 58.12 g/mol) / (0.0821 L*atm/mol*K * (27 + 273) K) = 2.21 g/L
Based on these calculations, the gas with a density of 2.32 g/L could be C4H10, which is option 4.