What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0 $\circ$ C?

Question

Quizplus · Accepted Answer

To find the molar mass of the gas, we can use the ideal gas law rearranged in terms of molar mass (M): M = (dRT)/(P), where d is the density, R is the ideal gas constant (0.0821 L·atm/(K·mol)), T is the temperature in Kelvin, and P is the pressure. First, convert the temperature from Celsius to Kelvin (25°C + 273.15 = 298.15 K). Then, plug in the values: M = (2.62 g/L * 0.0821 L·atm/(K·mol) * 298.15 K) / 2.00 atm = 32.0 g/mol.

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