Question

A sample of an unknown compound is vaporized at 190. °C. The gas produced has a volume of 2150. ml. at a pressure of 1.00 atm, and it weighs 7.77 g. 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.

          A sample of an unknown compound is vaporized at 190. °C. The gas produced has a volume of 2150. ml. at a pressure of 1.00 atm, and it weighs 7.77 g.
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.

A sample of an unknown compound is vaporized at 190. °C. The gas produced has a volume of 2150. ml. at a pressure of 1.00 atm, and it weighs 7.77 g.
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.

Added by Michael A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

08/20/2023

Step 1

00 atm) V = volume (2150 mL = 2.150 L) n = number of moles R = ideal gas constant (0.0821 L.atm/mol.K) T = temperature (190 K) Show more…

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help A sample of an unknown compound is vaporized at190.The gas produced has a volume of 2150.mL at a pressure of 1.00 atm,and it weighs 7.77 g. 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. mot X