4.500mL of an unknown organic liquid (SoecificGravity=0.785) was placed in a fla

Question

4.500mL of an unknown organic liquid (SoecificGravity=0.785) was placed in a flask and vaporized as in thisexperiment.

Data obtained follows: weight of vapor: 0.547g temperature of vapor:100 degrees C volume of vapor: 135mL pressure of vapor:765.2 torr a)Using the above data,calculate experimentalmolar mass. b)Calculate mL of the liquidcondensed. 4.500mL of an unknown organic liquid (SoecificGravity=0.785) was placed in a flask and vaporized as in thisexperiment.

Data obtained follows: weight of vapor: 0.547g temperature of vapor:100 degrees C volume of vapor: 135mL pressure of vapor:765.2 torr a)Using the above data,calculate experimentalmolar mass. b)Calculate mL of the liquidcondensed. b)Calculate mL of the liquidcondensed.

Explanation / Answer

Using, PV = nRT (Where P is pressure in atm, V is volume in Liters,n is number of moles, R is the gas constant .0821 L * atm/ mol * K,and T is temperature in kelvin), we can find how many moles of thegas was placed in the flask. First a few converstions: 100 C + 273.15 = 373.15 K 765.2/760 = 1.007 atm 135 mL = .135 Liters Now, plug in everything you know at this point into PV = nRT PV = nRT (1.007)(.135) = n(.0821)(373.15) Solving for n, we get n = .004437 moles Now that you know how many moles that are, we can find the molarmass using the weight of the vapor that was given. Since molar massis given by grams per mole, we can simply divide that mass by themole value we just found. 0.547 g/.004437 moles = 123.268 g/mol is the molarmass

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