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Answer :
The molar mass of the gaseous compound with a density of 1.37 g/L at 24.4 \\u00b0C and 1.73 atm is calculated to be 19.35 g/mol.
To find the molar mass of the gaseous compound, we can use the Ideal Gas Law equation in combination with the given density. The Ideal Gas Law is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. However, we will rearrange this to solve for the molar mass (M).
First, we convert the temperature from Celsius to Kelvin: T = 24.4 \\u00b0C + 273.15 = 297.55 K.
Next, we use the equation: M = (dRT)/P, where d is density. Remember to use R = 0.0821 L.atm.mol\\u207b\\u00b9.K\\u207b\\u00b9 for consistency in units.
We can calculate the molar mass as follows: M = (1.37 g/L * 0.0821 L.atm.mol\\u207b\\u00b9.K\\u207b\\u00b9 * 297.55 K) / 1.73 atm = 19.35 g/mol.
Therefore, the molar mass of the compound is 19.35 g/mol.
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