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A gaseous compound has a density of 1.70 g/L at 24.0°C and 1.61 atm. What is the molar mass of the compound?

Answer :

Final answer:

The molar mass of the gaseous compound can be calculated using the ideal gas law equation and the given conditions. After plugging in the values into the formula, the molar mass is found to be approximately 28.89 g/mol.

Explanation:

The molar mass of a gas can be calculated using the Ideal Gas Law equation and the equation for density (PM = dRT), where P is the pressure, M is the molar mass, d is the density, R is the universal gas constant, and T is the temperature in Kelvin. In this particular question, the density (d) is given as 1.70 g/L, the pressure (P) is 1.61 atm, and the temperature (T) needs to be converted from Celsius to Kelvin (24.0°C is 297.15 Kelvin). Also, R constant is given with a value of 0.0821 L·atm/mol·K in these units.

Plugging these values into the equation, we get:

Molar mass (M) = dRT/P = (1.70 g/L * 0.0821 L·atm/mol·K * 297.15 K) / 1.61 atm = 28.89 g/mole.

Therefore, the molar mass of the gaseous compound is approximately 28.89 g/mol.

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