Question

A sample of an unknown compound is vaporized at . The gas produced has a volume of at a pressure of , and it weighs . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits.

Answer 1

Answer:

The answer is "$34 \ \frac{g}{mol}$"

Explanation:

Please find the complete question in the attached file.

Formula:

$\to PV = nRT\\\\n = \frac{mass}{MW} \\\\PV = \frac{mRT}{MW}\\\\MW = \frac{mRT}{(PV)}\\\\MW = \frac{(0.941)(0.082)(150+273)}{(1 \times 0.96)}$

        $= \frac{(0.941)(0.082)(423)}{(0.96)} \\\\= \frac{32.639526}{(0.96)} \\\\= 33.9995062\ \ \ or \ \ \ 34 \ \frac{g}{mol}$