A sample of an unknown compound is vaporized at 170. °C. The gas produced has a volume of 1740. mL at a pressure of 1.00 atm, and it weighs 6.57 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. 0 8 mol X S

Chemistry: Principles and Practice
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter6: The Gaseous State
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A sample of an unknown compound is vaporized at 170. °C. The gas produced has a volume of 1740. mL at a pressure of 1.00 atm, and it weighs 6.57 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.
g
mol
0x1.²
X
Transcribed Image Text:A sample of an unknown compound is vaporized at 170. °C. The gas produced has a volume of 1740. mL at a pressure of 1.00 atm, and it weighs 6.57 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. g mol 0x1.² X
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