Answer :
Final answer:
The molar mass of the gaseous compound, calculated using the Ideal Gas Law and the given density, pressure, and temperature, is approximately 45 g/mol.
Explanation:
We can determine the molar mass of a gaseous compound using the Ideal Gas Law and the given information. The Ideal Gas Law equation is pV = nRT, where p stands for pressure, V for volume, n for number of moles, R for gas constant, and T for temperature in Kelvin. Using the law of physics that relates the density and molar mass of a gas, β = PMW/RT; where β is the density, P is the pressure, MW is the molar weight or molar mass, R the ideal gas constant, and T, the temperature.
We need to convert the temperature from Celsius to Kelvin by adding 273.15. That would be 297.35K. We rearrange the formula to solve for MW i.e., MW = βRT/P. Substituting in the known values we get: MW = (1.83g/L)*(0.0821 L.atm/mol.K)*(297.35K)/(1.69atm). The solution to this will give us the molar mass of the gaseous compound, which is approximately 45 g/mol.
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