# urgent due date is today

Aug 5th, 2015
Anonymous
Category:
Science
Price: \$10 USD

Question description

students calculate the molar mass(MM) of a volatile liquid using the ideal gas law (PV=nRT) IN  the following form:MM=(Mass of vapor*R* boiling point in kelvins)/(pressure in atmosphere*flask volume). if R=0.0821 liter-atmospheres/mole-degree K, the flask volume is 275 ml, and the pressure is 775 torr, calculate the following :the density of the vapor for CH2Cl2 at 75 degrees celsius and the EXPERIMENTAL molar mass of CCl4 if the mass of vapor in the flask is 1.44grams at 95 degrees celcius

PLEASE SHOW FULL WORK

(Top Tutor) Evans R.
School: Cornell University

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