Answer :

Final answer:

Using the density (1.30 g/L), temperature (26.5°C, converted to 299.65 K), and pressure (1.64 atm) provided, and the universal gas constant (0.0821 L*atm/K*mol), we can ascertain that the molar mass of the given gaseous compound is approximately 19.54 g/mol.

Explanation:

The question is asking for the molar mass of a gaseous compound with specific physical properties (density, temperature, pressure). The ideal gas law and molar mass could be applied to solve this question. We can resort to the equation for molar mass when physical properties of a gas are given:

Molar mass = (Density * R * T) / P

where:
R is the universal gas constant, which is 0.0821 L*atm/K*mol,
T is the temperature in Kelvin (K), which can be found by converting 26.5 °C to K (26.5 + 273.15 = 299.65 K),
P is the pressure of the gas in atm,

Plugging the given values into the equation:
Molar mass = (1.30 g/L * 0.0821 L*atm/K*mol * 299.65 K) / 1.64 atm = 19.54 g/mol

Therefore, the molar mass of the gaseous compound is approximately 19.54 g/mol.

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