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

The answer is "
`34 \ (g)/(mol)`"

Step-by-step explanation:

Please find the complete question in the attached file.

Formula:

`\to PV = nRT\\\\n = (mass)/(MW) \\\\PV = (mRT)/(MW)\\\\MW = (mRT)/((PV))\\\\MW = ((0.941)(0.082)(150+273))/((1 * 0.96))`

`= ((0.941)(0.082)(423))/((0.96)) \\\\= (32.639526)/((0.96)) \\\\= 33.9995062\ \ \ or \ \ \ 34 \ (g)/(mol)`