Question

Problem Page 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. Round your answer to significant digits. Clears your work. Undoes your last action. Provides information about entering answers.

Answer 1

138 g/mol

Step-by-step explanation:

There is some data missing. I think the original question is:

A sample of an unknown compound is vaporized at 130 °C. The gas produced has a volume of 960 mL at a pressure of 1.00 atm, and it weighs 3.99 g.

Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

First, we can find the moles of the gas using the ideal gas equation. (Absolute temperature 130 + 273 = 403 K)

`P.V=n.R.T\\n=(P.V)/(R.T) =((1.00atm).(0.960L))/((0.08206atm.L/mol.K).403K) =0.0290mol`

The molar mass of the compound is:

`M=(3.99g)/(0.0290mol) =138 g/mol`